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6. Chemical Quantities & Aqueous Reactions

Redox Reactions

6. Chemical Quantities & Aqueous Reactions

Redox Reactions

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Redox Reactions

Redox Reactions

Redox Reactions

Redox Reactions

Redox Reactions Example 1

Redox Reactions Example 1

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Oxidation-Reduction in Aqueous Solutions

Oxidation-Reduction in Aqueous Solutions

Introduction to Oxidation Reduction (Redox) Reactions

Introduction to Oxidation Reduction (Redox) Reactions

A Level Chemistry Revision "Introduction to Redox Reactions"

A Level Chemistry Revision "Introduction to Redox Reactions"

Freesciencelessons

What Are Redox Reactions? (Oxygen Exchange) | Reactions | Chemistry | FuseSchool

What Are Redox Reactions? (Oxygen Exchange) | Reactions | Chemistry | FuseSchool

FuseSchool - Global Education

Redox reactions

Redox reactions

Stile Education

GCSE Chemistry - Oxidation and Reduction - Redox Reactions #39 (Higher Tier)

GCSE Chemistry - Oxidation and Reduction - Redox Reactions #39 (Higher Tier)

Practice Problem: Balancing Redox Reactions

Practice Problem: Balancing Redox Reactions

Professor Dave Explains

Oxidation-Reduction Reactions

Oxidation-Reduction Reactions

Professor Dave Explains

Oxidation and Reduction (Redox) Reactions Step-by-Step Example

Oxidation and Reduction (Redox) Reactions Step-by-Step Example

Melissa Maribel

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Practice this topic

Multiple Choice

Which element is being reduced in the following reaction?

Cr₂O₇^2- + 3 HNO₂ + 5 H⁺→ 2 Cr³⁺ + 3NO₃^- + 4 H₂O

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Multiple Choice

Identify the oxidizing agent and reducing agent from the following redox reaction.

Ba (s) + Cl₂ (g) → BaCl₂ (aq)

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Multiple Choice

Which element is oxidized and which is reduced in the following reaction?

Hg (aq) + HgCl₂ (aq) → Hg₂Cl₂

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Multiple Choice

Which of the following represents an oxidation-reduction reaction?

I. PCl₃ (aq) + Cl₂ (g) → PCl₅ (aq)

II. 2 AgNO₃ (aq) + Cu (s) → Cu(NO₃)₂ (aq) + 2 Ag (s)

III. CO₂ (g) + 2 LiOH (aq) → Li₂CO₃ (aq) + H₂O (l)

IV. FeCl₂ (aq) + 2 NaOH (aq) → Fe(OH)₂ (aq) + 2 NaCl (aq)

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Multiple Choice

What is the oxidizing agent in the following reaction?

3 PbO (s) + 2 NH₃ (aq) → N₂ (g) + 3 H₂O (l) + 3 Pb (s)

Textbook Question

In the Brønsted–Lowry concept of acids and bases, acid– base reactions are viewed as proton-transfer reactions. The stronger the acid, the weaker is its conjugate base. If we were to think of redox reactions in a similar way, what particle would be analogous to the proton? Would strong oxidizing agents be analogous to strong acids or strong bases? [Sections 20.1 and 20.2]

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Textbook Question

The diagram that follows represents a molecular view of a process occurring at an electrode in a voltaic cell.

(c) Why are the atoms in the electrode represented by larger spheres than those in the solution? [Section 20.3]

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Textbook Question

What is the line notation for the galvanic cell?

(a) (b) (c) (d)

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Textbook Question

Consider the following voltaic cell:

(c) What is the change in the cell voltage when the ion concentrations in the cathode half-cell are increased by a factor of 10?

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Textbook Question

What is the pH of the solution in the cathode compartment of the following cell if the measured cell potential at 25 °C is 0.58 V? (Refer to Appendix B for standard reduction potentials.) (a) 8.0 (b) 4.5 (c) 2.2 (d) 3.0

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Textbook Question

Magnesium, the element, is produced commercially by electrolysis from a molten salt (the 'electrolyte') using a cell similar to the one shown here. (c) Recall that in an electrolytic cell the anode is given the + sign and the cathode is given the – sign, which is the opposite of what we see in batteries. What half-reaction occurs at the anode in this electrolytic cell?

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Textbook Question

Identify the element that gets oxidized and the oxidizing agent in the reaction. (LO 4.19) (a) (b) (c) (d)

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Textbook Question

(b) On which side of an oxidation half-reaction do the electrons appear?

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Textbook Question

What are the products of the overall reaction in the elec-trolysis of an aqueous solution of sodium hydroxide? (Refer to Table 19.1 for standard reduction potentials.) (a) Na(s) and O2(g) (b) H2(g) and O2(g) (c) Na(s) and H2(g) (d) Na(s) and H2O2(aq)

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Textbook Question

Indicate whether each of the following statements is true or false: (c) If there are no changes in the oxidation state of the reactants or products of a particular reaction, that reaction is not a redox reaction.

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Textbook Question

Indicate whether each of the following statements is true or false: (a) If something is oxidized, it is formally losing electrons.

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Textbook Question

Indicate whether each of the following statements is true or false: (c) An oxidizing agent is needed to convert CO into CO2.

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Textbook Question

Hydrazine 1N2H42 and dinitrogen tetroxide 1N2O42 form a self-igniting mixture that has been used as a rocket propellant. The reaction products are N2 and H2O. (c) Which substance serves as the reducing agent and which as the oxidizing agent?

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Textbook Question

(b) Write the half-reaction that occurs at a hydrogen electrode in acidic aqueous solution when it serves as the anode of a voltaic cell.

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Textbook Question

A voltaic cell that uses the reaction PdCl42-1aq2 + Cd1s2 ¡ Pd1s2 + 4 Cl-1aq2 + Cd2+1aq2 has a measured standard cell potential of +1.03 V. (b) By using data from Appendix E, determine E°red for the reaction involving Pd.

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Textbook Question

Consider a Daniell cell with 1.0 M ion concentrations:

Does the cell voltage increase, decrease, or remain the same when each of the following changes is made? Explain. (a) Write a balanced equation for each cell reaction.

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Textbook Question

Using standard reduction potentials (Appendix E), calculate the standard emf for each of the following reactions: (c) Fe1s2 + 2 Fe3+1aq2 ¡ 3 Fe2+1aq2

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Textbook Question

Using standard reduction potentials (Appendix E), calculate the standard emf for each of the following reactions: (b) Ni1s2 + 2 Ce4+1aq2 ¡ Ni2+1aq2 + 2 Ce3+1aq2

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Textbook Question

Using standard reduction potentials (Appendix E), calculate the standard emf for each of the following reactions: (a) Cl21g2 + 2 I-1aq2 ¡ 2 Cl-1aq2 + I21s2

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Textbook Question

Using standard reduction potentials (Appendix E), calculate the standard emf for each of the following reactions: (d) 2 NO3-1aq2 + 8 H+1aq2 + 3 Cu1s2 ¡ 2 NO1g2 + 4 H2O1l2 + 3 Cu2+1aq2

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Textbook Question

Sketch a cell with inert electrodes suitable for electrolysis of aqueous CuBr2. (b) Indicate the direction of electron and ion flow.

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Textbook Question

The standard reduction potentials of the following halfreactions are given in Appendix E: Ag+1aq2 + e- ¡ Ag1s2 Cu2+1aq2 + 2 e- ¡ Cu1s2 Ni2+1aq2 + 2 e- ¡ Ni1s2 Cr3+1aq2 + 3 e- ¡ Cr1s2 (b) Determine which combination of these half-cell reactions leads to the cell reaction with the smallest positive cell potential and calculate the value.

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Textbook Question

Porous pellets of TiO2 can be reduced to titanium metal at the cathode of an electrochemical cell containing molten CaCl2 as the electrolyte. When the TiO2 is reduced, the O2-ions dis-solve in the CaCl2 and are subsequently oxidized to O2 gas at the anode. This approach may be the basis for a less expensive process than the one currently used for producing titanium.

(c) Write balanced equations for the anode, cathode, and overall cell reactions.

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Textbook Question

Calculate the standard cell potential for each of the electro- chemical cells in Problem 43.

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Textbook Question

True or false: (a) If a substance is oxidized, there must be more oxygen in the substance.

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Textbook Question

True or false: (a) Reduction occurs if the oxidation number of an element increases

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Textbook Question

(a) Which region of the periodic table shown here contains elements that are easiest to oxidize? (b) Which region contains the least readily oxidized elements?

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Textbook Question

Use line notation to represent each electrochemical cell in Problem 43.

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Textbook Question

Make a sketch of the voltaic cell represented by the line nota- tion. Write the overall balanced equation for the reaction and calculate Ec°ell. Sn(s) | Sn2+(aq) || NO( g) | NO3-(aq), H+(aq) | Pt(s)

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Textbook Question

Which element is oxidized, and which is reduced in the following reactions? (c) Cl21aq2 + 2 NaI1aq2¡I21aq2 + 2 NaCl1aq2

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Textbook Question

Which element is oxidized, and which is reduced in the following reactions? (b) 3 Fe1NO3221aq2 + 2 Al1s2¡3 Fe1s2 + 2 Al1NO3231aq2

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Textbook Question

Which element is oxidized, and which is reduced in the following reactions? (a) N21g2 + 3 H21g2¡2 NH31g2

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Textbook Question

For each of the following reactions, write a balanced equation, calculate the standard emf, calculate ∆G° at 298 K, and calculate the equilibrium constant K at 298 K. (c) In basic solution, Cr1OH231s2 is oxidized to CrO42-1aq2 by ClO-1aq2.

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Textbook Question

For each of the following reactions, write a balanced equation, calculate the standard emf, calculate ∆G° at 298 K, and calculate the equilibrium constant K at 298 K. (a) Aqueous iodide ion is oxidized to I21s2 by Hg22+1aq2.

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Textbook Question

Which of the following are redox reactions? For those that are, indicate which element is oxidized and which is reduced. For those that are not, indicate whether they are precipitation or neutralization reactions. (a) P41s2 + 10 HClO1aq2 + 6 H2O1l2¡ 4 H3PO41aq2 + 10 HCl1aq2

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Textbook Question

For each of the following reactions, write a balanced equation, calculate the standard emf, calculate ∆G° at 298 K, and calculate the equilibrium constant K at 298 K. (b) In acidic solution, copper(I) ion is oxidized to copper(II) ion by nitrate ion.

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Textbook Question

Determine whether or not each redox reaction occurs spontaneously in the forward direction. a. Ni(s) + Zn2+(aq) ¡ Ni2+(aq) + Zn(s)

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Textbook Question

Determine whether or not each redox reaction occurs spontaneously in the forward direction. b. 2 Ag+(aq) + Ni(s) ¡ 2 Ag(s) + Ni2+(aq)

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Textbook Question

Using the standard reduction potentials listed in Appendix E, calculate the equilibrium constant for each of the following reactions at 298 K: (c) 10 Br -1aq2 + 2 MnO4-1aq2 + 16 H+1aq2 ¡ 2 Mn2+1aq2 + 8 H2O1l2 + 5 Br21l2

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Textbook Question

A cell has a standard cell potential of +0.177 V at 298 K. What is the value of the equilibrium constant for the reaction (c) if n = 3?

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Textbook Question

Write a balanced equation for the overall cell reaction in the following galvanic cell, and tell why inert electrodes are required at the anode and cathode. Pt(s) | Br-(aq) | Br2(l2) || Cl2(g) | Cl-(aq) || Pt(s)

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Textbook Question

Write the shorthand notation for a galvanic cell that uses the following cell reaction. Include inert electrodes if necessary. 2 Fe1s2 + Cr2O72-1aq2 + 14 H+1aq2¡2 Fe3+1aq2 + 2 Cr3+1aq2 + 7 H2O1l2

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Textbook Question

Calculate Ec°ell for each balanced redox reaction and determine if the reaction is spontaneous as written. b. MnO2(aq) + 4 H+(aq) + Zn(s) ¡ Mn2+(aq) + 2H2O(l) + Zn2+(aq)

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Textbook Question

Calculate Ec°ell for each balanced redox reaction and determine if the reaction is spontaneous as written. a. 2 Cu(s) + Mn2+(aq) ¡ 2 Cu+(aq) + Mn(s)

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Textbook Question

An H2/H+ half-cell (anode) and an Ag+/Ag half cell (cathode) are connected by a wire and a salt bridge. (a) Sketch the cell, indicating the direction of electron and ion flow.

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Textbook Question

An H2/H+ half-cell (anode) and an Ag+/Ag half cell (cathode) are connected by a wire and a salt bridge. (c) Give the shorthand notation for the cell.

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Textbook Question

Calculate Ec°ell for each balanced redox reaction and determine if the reaction is spontaneous as written. c. PbO2(s) + 4 H+(aq) + Sn(s) ¡ Pb2+(aq) + 2H2O(l) + Sn2+(aq)

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Textbook Question

Calculate Ec°ell for each balanced redox reaction and determine if the reaction is spontaneous as written. a. O2(g) + 2 H2O(l) + 4 Ag(s) ¡ 4 OH-(aq) + 4 Ag+(aq)

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Textbook Question

Write balanced equations for the electrode and overall cell reactions in the following galvanic cells. Sketch each cell, labeling the anode and cathode and showing the direction of electron and ion flow. (a) .

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Textbook Question

A voltaic cell utilizes the following reaction: Al1s2 + 3 Ag+1aq2 ¡ Al3+1aq2 + 3 Ag1s2 What is the effect on the cell emf of each of the following changes? (a) Water is added to the anode half-cell, diluting the solution.

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Textbook Question

A voltaic cell is constructed that uses the following reaction and operates at 298 K: Zn1s2 + Ni2+1aq2 ¡ Zn2+1aq2 + Ni1s2 (c) What is the emf of the cell when 3Ni2+4 = 0.200 M and 3Zn2+4 = 0.900 M?

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Textbook Question

A voltaic cell utilizes the following reaction: 4 Fe2+1aq2 + O21g2 + 4 H+1aq2 ¡ 4 Fe3+1aq2 + 2 H2O1l2 (a) What is the emf of this cell under standard conditions?

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Textbook Question

A voltaic cell utilizes the following reaction: 4 Fe2+1aq2 + O21g2 + 4 H+1aq2 ¡ 4 Fe3+1aq2 + 2 H2O1l2 (b) What is the emf of this cell when 3Fe2+4 = 1.3 M, 3Fe3+4= 0.010 M, PO2 = 0.50 atm, and the pH of the solution in the cathode half-cell is 3.50?

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Textbook Question

Calculate the equilibrium constant for each of the reactions in Problem 65.

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Textbook Question

A voltaic cell utilizes the following reaction: 2 Fe3+1aq2 + H21g2 ¡ 2 Fe2+1aq2 + 2 H+1aq2 (a) What is the emf of this cell under standard conditions?

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Textbook Question

A voltaic cell utilizes the following reaction: (b) What is the emf for this cell when 3Fe3+4 = 3.50 M, PH2= 0.95 atm, 3Fe2+4 = 0.0010 M, and the pH in both half-cells is 4.00?

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Textbook Question

Calculate the equilibrium constant for the reaction between Fe2+(aq) and Zn(s) (at 25 °C).

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Textbook Question

A voltaic cell is constructed that is based on the following reaction: Sn2+1aq2 + Pb1s2 ¡ Sn1s2 + Pb2+1aq2 (a) If the concentration of Sn2+ in the cathode half-cell is 1.00 M and the cell generates an emf of +0.22 V, what is the concentration of Pb2+ in the anode half-cell?

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Textbook Question

A voltaic cell employs the following redox reaction: Sn2+(aq) + Mn(s) ¡ Sn(s) + Mn2+(aq) Calculate the cell potential at 25 °C under each set of conditions. c. [Sn2+] = 2.00 M; [Mn2+] = 0.0100 M

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Textbook Question

During the discharge of an alkaline battery, 4.50 g of Zn is consumed at the anode of the battery. (b) How many coulombs of electrical charge are transferred from Zn to MnO2?

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Textbook Question

Heart pacemakers are often powered by lithium–silver chromate 'button' batteries. The overall cell reaction is 2 Li1s2 + Ag2CrO41s2 ¡ Li2CrO41s2 + 2 Ag1s2 (b) Choose the two half-reactions from Appendix E that most closely approximate the reactions that occur in the battery. What standard emf would be generated by a voltaic cell based on these half-reactions?

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Textbook Question

An electrochemical cell is based on these two half-reactions: Ox: Pb(s) -> Pb2+ (aq, 0.10 M) + 2 e- Red: MnO4-(aq, 1.50 M) + 4 H+(aq, 2.0 M) + 3 e- -> MnO2(s) + 2 H2O(l) Calculate the cell potential at 25 °C.

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Textbook Question

An electrochemical cell is based on these two half-reactions: Ox: Sn(s) ¡ Sn2+(aq, 2.00 M) + 2 e- Red: ClO2(g, 0.100 atm) + e- ¡ ClO2-(aq, 2.00 M) Calculate the cell potential at 25 °C.

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Textbook Question

A voltaic cell consists of a Zn>Zn2+ half-cell and a Ni>Ni2+ half-cell at 25 °C. The initial concentrations of Ni2+ and Zn2+ are 1.50 M and 0.100 M, respectively. c. What are the concentrations of Ni2+ and Zn2+ when the cell potential falls to 0.45 V? Ec°ell for the fuel-cell breathalyzer, which employs the following

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Textbook Question

A voltaic cell consists of a Zn>Zn2+ half-cell and a Ni>Ni2+ half-cell at 25 °C. The initial concentrations of Ni2+ and Zn2+ are 1.50 M and 0.100 M, respectively. b. What is the cell potential when the concentration of Ni2+ has fallen to 0.500 M?

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Textbook Question

A voltaic cell consists of a Zn>Zn2+ half-cell and a Ni>Ni2+ half-cell at 25 °C. The initial concentrations of Ni2+ and Zn2+ are 1.50 M and 0.100 M, respectively. a. What is the initial cell potential?

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Textbook Question

Consider the following substances: Fe(s), PbO2(s), H+(aq), Al(s), Ag(s), Cr2O72-(aq). (a) Look at the E° values in Appendix D, and classify each substance as an oxidizing agent or a reducing agent.

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Textbook Question

A voltaic cell consists of a Pb>Pb half-cell and a Cu>Cu half- cell at 25°C. The initial concentrations of Pb2+ and Cu2+ are 0.0500 M and 1.50 M, respectively. c. What are the concentrations of Pb2+ and Cu2+ when the cell potential falls to 0.35 V?

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Textbook Question

A voltaic cell consists of a Pb>Pb half-cell and a Cu>Cu half- cell at 25°C. The initial concentrations of Pb2+ and Cu2+ are 0.0500 M and 1.50 M, respectively. b. What is the cell potential when the concentration of Cu2+ has fallen to 0.200 M?

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Textbook Question

A voltaic cell consists of a Pb>Pb half-cell and a Cu>Cu half- cell at 25°C. The initial concentrations of Pb2+ and Cu2+ are 0.0500 M and 1.50 M, respectively. a. What is the initial cell potential?

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Textbook Question

The following cell reactions occur spontaneously: (c) Which of the three cell reactions delivers the highest voltage?

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Textbook Question

The following cell reactions occur spontaneously: (a) Arrange the following reduction half-reactions in order of decreasing tendency to occur:

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Textbook Question

The following cell reactions occur spontaneously: (b) Which of these substances (A,A+,B,B+,C,C+) is the strongest oxidizing agent? Which is the strongest reducing agent?

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Textbook Question

Use the data in Appendix D to predict whether the following reactions can occur under standard-state conditions. (d) Reduction of I2(s) by H2SO3(aq)

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Textbook Question

Use the data in Appendix D to predict whether the following reactions can occur under standard-state conditions. (c) Oxidation of Ag(s) by Pb2+(aq)

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Textbook Question

Use the data in Appendix D to predict whether the following reactions can occur under standard-state conditions. (b) Reduction of Ni2+(aq) by Sn2+(aq)

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Textbook Question

(a) Which reaction is spontaneous in the hydrogen fuel cell: hydrogen gas plus oxygen gas makes water, or water makes hydrogen gas plus oxygen gas?

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Textbook Question

A concentration cell consists of two Sn/Sn2+ half-cells. The cell has a potential of 0.10 V at 25°C. What is the ratio of the Sn2+ concentrations in the two half-cells?

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Textbook Question

What reaction can occur, if any, when the following experiments are carried out under standard-state conditions? (d) A nickel wire is dipped into an aqueous solution of HClO.

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Textbook Question

What reaction can occur, if any, when the following experiments are carried out under standard-state conditions? (c) Chlorine gas is bubbled through aqueous H2C2O4.

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Textbook Question

What reaction can occur, if any, when the following experiments are carried out under standard-state conditions? (b) A strip of lead is dipped into an aqueous solution of AgNO3.

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Textbook Question

What reaction can occur, if any, when the following experiments are carried out under standard-state conditions? (a) Oxygen gas is bubbled through an acidic solution of Cr(NO3)3.

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Textbook Question

A Cu/Cu2+ concentration cell has a voltage of 0.22 V at 25 °C. The concentration of Cu2+ in one of the half-cells is 1.5x10^-3 M. What is the concentration of Cu2+ in the other half-cell? (Assume the concentration in the unknown cell is the lower of the two concentrations.)

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Textbook Question

What reaction can occur, if any, when the following experiments are carried out under standard-state conditions? (b) An acidic solution of FeSO4 is exposed to oxygen.

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Textbook Question

What reaction can occur, if any, when the following experiments are carried out under standard-state conditions? (d) Hydrogen gas is bubbled through aqueous Cd(NO3)2.

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Textbook Question

What reaction can occur, if any, when the following experiments are carried out under standard-state conditions? (c) A silver wire is immersed in an aqueous solution of NiCl2.

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Textbook Question

What reaction can occur, if any, when the following experiments are carried out under standard-state conditions? (a) A strip of zinc is dipped into an aqueous solution of Pb(NO3)2.

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Textbook Question

The standard potential for the following galvanic cell is 0.40 V: (Europium, Eu, is one of the lanthanide elements.) Use the data in Table 19.1 to calculate the standard reduction potential for Eu3+/Eu2+ half-cell.

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Textbook Question

Refer to the tabulated values of ∆Gf° in Appendix IIB to calculate Ec°ell for the fuel-cell breathalyzer, which employs the following reaction. ((∆G° for HC H O (g) = -374.2 kJ>mol.) CH3CH2OH(g) + O2(g) ¡ HC2H3O2(g) + H2O(g)

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Textbook Question

Determine whether or not each metal, if coated onto iron, would prevent the corrosion of iron. c. Mn

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Textbook Question

Determine whether or not each metal, if coated onto iron, would prevent the corrosion of iron. b. Sn

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Textbook Question

Determine whether or not each metal, if coated onto iron, would prevent the corrosion of iron. a. Zn

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Textbook Question

Determine whether or not each metal, if coated onto iron, would prevent the corrosion of iron. c. Cu

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Textbook Question

Determine whether or not each metal, if coated onto iron, would prevent the corrosion of iron. a. Mg

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Textbook Question

Determine whether or not each metal, if coated onto iron, would prevent the corrosion of iron. b. Cr

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Textbook Question

(d) Why is sodium metal not obtained when an aqueous solution of NaCl undergoes electrolysis?

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Textbook Question

(c) What process occurs at the anode in the electrolysis of molten NaCl?

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Textbook Question

(d) Why are active metals such as Al obtained by electrolysis using molten salts rather than aqueous solutions?

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Textbook Question

Draw an electrolytic cell in which Mn2+ is reduced to Mn and Sn is oxidized to Sn2+. Label the anode and cathode, indicate the direction of electron flow, and write an equation for the half- reaction occurring at each electrode. What minimum voltage is necessary to drive the reaction?

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Textbook Question

Calculate E° for each of the following reactions, and tell which are spontaneous under standard-state conditions. (a)

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Textbook Question

Write equations for the half-reactions that occur in the electrol- ysis of molten potassium bromide.

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Textbook Question

(a) A Cr3+1aq2 solution is electrolyzed, using a current of 7.60 A. What mass of Cr(s) is plated out after 2.00 days?

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Textbook Question

Consider a galvanic cell that uses the following half-reactions: (b) What is the oxidizing agent, and what is the reducing agent?.

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Textbook Question

What products are obtained in the electrolysis of molten NaI?

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Textbook Question

The accompanying photo shows the reaction between a solution of Cd1NO322 and one of Na2S. (d) Is this a redox reaction?

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Textbook Question

Given the following half-reactions and E° values, write a balanced equation for the formation of Mn2+ and MnO2 from Mn3+, and calculate the value of E° for this reaction. Is the reaction spontaneous under standard-state conditions?

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Textbook Question

(a) Calculate the mass of Li formed by electrolysis of molten LiCl by a current of 7.5 * 104 A flowing for a period of 24 h. Assume the electrolytic cell is 85% efficient. (b) What is the minimum voltage required to drive the reaction?

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Textbook Question

What products are obtained in the electrolysis of a molten mix- ture of KI and KBr?

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Textbook Question

Consider a galvanic cell that uses the reaction Calculate the potential at 25 °C for a cell that has the following ion concentrations: [Ag+] = 0.010M, [Ni2+] = 0.100M.

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Textbook Question

The commercial production of nitric acid involves the following chemical reactions: 4 NH31g2 + 5 O21g2¡4 NO1g2 + 6 H2O1g2 2 NO1g2 + O21g2¡2 NO21g2 3 NO21g2 + H2O1l2¡2 HNO31aq2 + NO1g2 (b) Identify the element undergoing oxidation and the element undergoing reduction. 3 NO21g2 + H2O1l2¡2 HNO31aq2 + NO1g2

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Textbook Question

Write equations for the half-reactions that occur at the anode and cathode for the electrolysis of each aqueous solution. a. Ni(NO3)2(aq)

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Textbook Question

The commercial production of nitric acid involves the following chemical reactions: 4 NH31g2 + 5 O21g2¡4 NO1g2 + 6 H2O1g2 2 NO1g2 + O21g2¡2 NO21g2 3 NO21g2 + H2O1l2¡2 HNO31aq2 + NO1g2 (a) Which of these reactions are redox reactions?

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Textbook Question

Determine whether each reaction is a redox reaction. For each redox reaction, identify the oxidizing agent and the reducing agent. c. Pb(NO3)2(aq) + Na2SO4(aq)¡PbSO4(s) + 2 NaNO3(aq) d. HBr(aq) + KOH(aq)¡H2O(l ) + KBr(aq)

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Textbook Question

Determine whether each reaction is a redox reaction. For each redox reaction, identify the oxidizing agent and the reducing agent. a. 4 Li(s) + O2( g)¡2 Li2O(s) b. Mg(s) + Fe2 + (aq)¡Mg2 + (aq) + Fe(s)

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Textbook Question

A galvanic cell has an iron electrode in contact with 0.10 M FeSO4 and a copper electrode in contact with a CuSO4 solu-tion. If the measured cell potential at 25 °C is 0.67 V, what is the concentration of Cu2+ in the CuSO4 solution?

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Textbook Question

Determine whether each reaction is a redox reaction. For each redox reaction, identify the oxidizing agent and the reducing agent. a. Al(s) + 3 Ag+ (aq)¡Al3 + (aq) + 3 Ag(s) b. SO3( g) + H2O(l )¡H2SO4(aq) c. Ba(s) + Cl2( g)¡BaCl2(s) d. Mg(s) + Br2(l )¡MgBr2(s)

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Textbook Question

What is the Fe2+: Sn2+ concentration ratio in the following cell at 25 °C if the measured cell potential is 0.35 V?

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Textbook Question

Predict whether the following reactions will be spontaneous in acidic solution under standard conditions: (c) reduction of Ce4+ to Ce3+ by H2O2,

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Textbook Question

The Nernst equation applies to both cell reactions and half-reactions. For the conditions specified, calculate the potential for the following half-reactions at 25 °C. (b)

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Textbook Question

Gold exists in two common positive oxidation states, +1 and +3. The standard reduction potentials for these oxidation states are Au+1aq2 + e- ¡ Au1s2 Ered ° = +1.69 V Au3+1aq2 + 3 e- ¡ Au1s2 Ered ° = +1.50 V (c) Miners obtain gold by soaking gold-containing ores in an aqueous solution of sodium cyanide. A very soluble complex ion of gold forms in the aqueous solution because of the redox reaction 4 Au1s2 + 8 NaCN1aq2 + 2 H2O1l2 + O21g2 ¡ 4 Na3Au1CN2241aq2 + 4 NaOH1aq2 What is being oxidized, and what is being reduced in this reaction?

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Textbook Question

Silver can be electroplated at the cathode of an electrolysis cell by the half-reaction: Ag+(aq) + e- ¡ Ag(s) What mass of silver would plate onto the cathode if a current of 6.8 A flowed through the cell for 72 min?

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Textbook Question

When suspected drunk drivers are tested with a Breathalyzer, the alcohol (ethanol) in the exhaled breath is oxidized to acetic acid with an acidic solution of potassium dichromate: The color of the solution changes because some of the orange Cr2O7 2-is converted to the green Cr3+ The Breath-alyzer measures the color change and produces a meter reading calibrated in blood alcohol content. (b) What is the value of E for the reaction when the concentrations of ethanol, acetic acid, Cr2O7 are 1.0 M and the pH is 4.00?

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Textbook Question

When suspected drunk drivers are tested with a Breathalyzer, the alcohol (ethanol) in the exhaled breath is oxidized to acetic acid with an acidic solution of potassium dichromate: The color of the solution changes because some of the orange Cr2O7 2-is converted to the green Cr3+ The Breath-alyzer measures the color change and produces a meter reading calibrated in blood alcohol content. (a) What is E° for the reaction if the standard half-cell potential for the reduction of acetic acid to ethanol is 0.058 V?

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Textbook Question

A major source of sodium metal is the electrolysis of molten so- dium chloride. What magnitude of current produces 1.0 kg of sodium metal in 1 hour?

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Textbook Question

A voltaic cell is constructed that uses the following half-cell reactions: Cu+1aq2 + e- ¡ Cu1s2 I21s2 + 2 e- ¡ 2 I-1aq2 The cell is operated at 298 K with 3Cu+4 = 0.25 M and 3I-4 = 0.035 M. (a) Determine E for the cell at these concentrations.

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Textbook Question

At one time on Earth, iron was present mostly as iron(II). Later, once plants had produced a significant quantity of oxygen in the atmosphere, the iron became oxidized to iron(III). Show that Fe2+(aq) can be spontaneously oxidized to Fe3+(aq) by O2(g) at 25°C assuming the following reasonable environmental conditions:

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Textbook Question

Consider the reaction shown here occurring at 25 °C. Cr(s) + Cd2+(aq) ¡ Cr2+(aq) + Cd(s) Determine Ec°ell, K, and ∆Gr°xn for the reaction and complete the table. [Cd2+] [Cr2+] Q Ecell 𝚫Grxn 1.00 1.00 1.00 * 10-5 4.18 * 10-4 1.00 1.00 * 10-5 1.00 1.00

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Textbook Question

(b) Given the following reduction potentials, calculate the standard emf of the cell: Cd1OH221s2 + 2 e- ¡ Cd1s2 + 2 OH-1aq2 E°red = -0.76 V NiO1OH21s2 + H2O1l2 + e- ¡ Ni1OH221s2 + OH-1aq2 E°red = +0.49 V

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Textbook Question

Copper reduces dilute nitric acid to nitric oxide (NO) but reduces concentrated nitric acid to nitrogen dioxide (NO2): Assuming that [Cu2+] = 0.10 M and that the partial pressures of NO and NO2 are 1.0 * 10-3 atm, calculate the potential (E) for reactions (1) and (2) at 25 °C and show which reaction has the greater thermodynamic tendency to occur when the concentration of HNO3 is (a) 1.0 M

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Textbook Question

Disulfides are compounds that have S ¬ S bonds, like peroxides have O ¬ O bonds. Thiols are organic compounds that have the general formula R ¬ SH, where R is a generic hydrocarbon. The SH- ion is the sulfur counterpart of hydroxide, OH-. Two thiols can react to make a disulfide, R ¬ S ¬ S ¬ R. (c) If you react two thiols to make a disulfide, are you oxidizing or reducing the thiols?

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Textbook Question

What is the pH of the solution in the cathode compartment of the following cell if the measured cell potential at 25 °C is 0.17 V?

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Textbook Question

Beginning with the equations that relate E°, ∆G°, and K, show that ∆G° is negative and K 7 1 for a reaction that has a positive value of E°

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Textbook Question

If a reaction has an equilibrium constant K 6 1, is E° posi-tive or negative? What is the value of K when E° = 0 V?

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Textbook Question

Calculate the number of kilowatt-hours of electricity required to produce 1.0 * 103 kg (1 metric ton) of aluminum by electrolysis of Al3+ if the applied voltage is 4.50 V and the process is 45% efficient.

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Textbook Question

The cell potential of this electrochemical cell depends on the gold concentration in the cathode half-cell. Pt(s) | H2(g, 1.0 atm) | H+(aq, 1.0 M) || Au3+(aq, ? M) | Au(s) What is the concentration of Au3+ in the solution if Ecell is 1.22 V?

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Textbook Question

Aqueous solutions of ammonia 1NH32 and bleach (active ingredient NaOCl) are sold as cleaning fluids, but bottles of both of them warn: 'Never mix ammonia and bleach, as toxic gases may be produced.' One of the toxic gases that can be produced is chloroamine, NH2Cl. (e) Is N oxidized, reduced, or neither, upon the conversion of ammonia to nitrogen trichloride?

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Textbook Question

Where in the periodic table are the best reducing agents found? The best oxidizing agents?

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Textbook Question

Where in the periodic table are the most easily reduced elements found? The most easily oxidized?

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Textbook Question

A battery relies on the oxidation of magnesium and the reduction of Cu2+. The initial concentrations of Mg2+ and Cu2+ are 1.0 * 10-4 M and 1.5 M, respectively, in 1.0-liter half-cells. a. What is the initial voltage of the battery?

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Textbook Question

Potassium superoxide, KO2, is often used in oxygen masks (such as those used by firefighters) because KO2 reacts with CO2 to release molecular oxygen. Experiments indicate that 2 mol of KO21s2 react with each mole of CO21g2. (b) Indicate the oxidation number for each atom involved in the reaction in part (a). What elements are being oxidized and reduced?

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Textbook Question

In each of the following instances, tell whether the substance gains electrons or loses electrons in a redox reaction. (a) An oxidizing agent (b) A reducing agent (c) A substance undergoing oxidation (d) A substance undergoing reduction

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Textbook Question

The following galvanic cell has a potential of 1.214 V at 25 °C: Calculate the value of Ksp for Hg2Br2 at 25°C

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Textbook Question

For the following half-reaction, E° = 1.103 V: Calculate the formation constant Kf for Cu(CN)2-.

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Textbook Question

Tell for each of the following substances whether the oxidation number increases or decreases in a redox reaction. (a) An oxidizing agent (b) A reducing agent (c) A substance undergoing oxidation (d) A substance undergoing reduction

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Textbook Question

Which element is oxidized and which is reduced in each of the following reactions? (b)

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Textbook Question

Which element is oxidized and which is reduced in each of the following reactions? (a)

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Textbook Question

Which element is oxidized and which is reduced in each of the following reactions? (b)

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Textbook Question

Which element is oxidized and which is reduced in each of the following reactions? (a)

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Textbook Question

A student designs an ammeter (a device that measures electrical current) that is based on the electrolysis of water into hydrogen and oxygen gases. When electrical current of unknown magnitude is run through the device for 2.00 min, 12.3 mL of water-saturated H21g2 is collected. The temperature of the system is 25.5 °C, and the atmospheric pressure is 768 torr. What is the magnitude of the current in amperes?

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Textbook Question

Treatment of gold metal with BrF3 and KF produces Br2 and KAuF4, a salt of gold. Identify the oxidizing agent and the reducing agent in this reaction.

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Textbook Question

You are on your dream vacation at the beach when a major storm knocks out the power for days. Your cell phone is dead, and you want to make a battery to charge it. You find the following materials in the beach house. blue stone algaecide for pools, which can be used to make a 1.0 M Cu2+ solution alum in the kitchen, which can be used to make a 1.0 M Al3+ solution aluminum foil, copper wire, and bologna, which can be used as a salt bridge. (b) What voltage can be generated?

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Textbook Question

You are on your dream vacation at the beach when a major storm knocks out the power for days. Your cell phone is dead, and you want to make a battery to charge it. You find the following materials in the beach house. blue stone algaecide for pools, which can be used to make a 1.0 M Cu2+ solution alum in the kitchen, which can be used to make a 1.0 M Al3+ solution aluminum foil, copper wire, and bologna, which can be used as a salt bridge. (d) An iPhone requires 5.0 V for charging. Can this battery charge the phone? Explain.

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Textbook Question

A storm has knocked out power to your beach house, and you would like to build a battery from household items to charge your iPhone. You have the following materials. alum in the kitchen, which can be used to make a 1.0 M Al3+ solution bleach, which is a solution that is approximately a 1.0 M in ClO-aluminum foil, a platinum necklace and bologna, which can be used as a salt bridge (b) What voltage can be generated?

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Textbook Question

Calculate ∆Gr°xn and K for each reaction. b. The reaction of Cr3+(aq) and Cr(s) to form Cr2+(aq). [The electrode potential of Cr2+(aq) to Cr(s) is -0.91 V.]

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Textbook Question

Calculate ∆Gr°xn and K for each reaction. a. The reaction of Cr2+(aq) with Cr2O7^2-(aq) in acid solution to form Cr3+(aq).

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Textbook Question

A mercury battery uses the following electrode half-reactions: (c) What is the effect on the cell voltage of a tenfold change in the concentration of KOH in the electrolyte? Explain..

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Textbook Question

A mercury battery uses the following electrode half-reactions: (b) Calculate ∆G° (in kilojoules) and K at 25 °C for the cell reaction.

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Textbook Question

A metal forms the fluoride MF3. Electrolysis of the molten fluo- ride by a current of 3.86 A for 16.2 minutes deposits 1.25 g of the metal. Calculate the molar mass of the metal.

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Textbook Question

A sample of impure tin of mass 0.535 g is dissolved in strong acid to give a solution of Sn2+. The solution is then titrated with a 0.0448 M solution of NO3-, which is reduced to NO(g). The equivalence point is reached upon the addition of 0.0344 L of the NO3- solution. Find the percent by mass of tin in the original sample, assuming that it contains no other reducing agents.

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Textbook Question

How does the pH of the solution affect the formation of rust?

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Textbook Question

Which of the following describes the process of galvanization that protects steel from rusting? (a) Steel is coated with a layer of paint. (b) Iron in steel is oxidized to form a protective oxide coating. (c) Steel is coated with zinc because zinc is more easily oxidized than iron. (d) A strip of magnesium is attached to steel because the magnesium is more easily oxidized than iron.

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Textbook Question

A current of 11.3 A is applied to 1.25 L of a solution of 0.552 M HBr converting some of the H+ to H2(g), which bubles out of solution. What is the pH of the solution after 73 minutes?

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Textbook Question

What is meant by cathodic protection? (a) Steel is coated with a layer of paint. (b) Iron in steel is oxidized to form a protective oxide coating. (c) Steel is coated with zinc because zinc is more easily oxidized than iron. (d) A strip of magnesium is attached to steel because the magnesium is more easily oxidized than iron.

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Textbook Question

An MnO2(s)/Mn2+(aq) electrode in which the pH si 10.24 is prepared. Find the [Mn2+] necessary to lower the potential of the half-cell to 0.00 V (at 25°C)

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Textbook Question

Which of the following metals can offer cathodic protec-tion to iron? Select all the correct choices. Mn, Ni, Pb, Sn, Al

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Textbook Question

To what pH should you adjust a standard hydrogen electrode to get an electrode potential of -0.122 V? (Assume that the partial pressure of hydrogen gas remains at 1 atm.)

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Textbook Question

Magnesium metal is produced by the electrolysis of molten magnesium chloride using inert electrodes. (a) Sketch the cell, label the anode and cathode, indicate the sign of the electrodes, and show the direction of electron and ion flow.

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Textbook Question

(a) Sketch a cell with inert electrodes suitable for the elec-trolysis of an aqueous solution of sulfuric acid. Label the anode and cathode, and indicate the direction of electron and ion flow. Identify the positive and negative electrodes. (b) Write balanced equations for the anode, cathode, and overall cell reactions.

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Textbook Question

What products should be formed when the following reac-tants are electrolyzed in a cell having inert electrodes? Account for any differences. (b) Aqueous KCl

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Textbook Question

Predict the anode, cathode, and overall cell reactions when an aqueous solution of each of the following salts is electrolyzed in a cell having inert electrodes. (b) CuCl2

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Textbook Question

Predict the anode, cathode, and overall cell reactions when an aqueous solution of each of the following salts is electrolyzed in a cell having inert electrodes. (c) LiOH

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Textbook Question

Predict the anode, cathode, and overall cell reactions when an aqueous solution of each of the following salts is electrolyzed in a cell having inert electrodes. (a) Ag2SO4

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Textbook Question

What constant current (in amperes) is required to produce aluminum by the Hall–Héroult process at a rate of 40.0 kg/h?

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Textbook Question

Electrolysis of a metal nitrate solution M(NO3)2(aq) for 325 min with a constant current of 20.0 A gives 111 g of the metal. Identify the metal ion M2+.

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Textbook Question

Aluminum, titanium, and several other metals can be col-ored by an electrochemical process called anodizing. Anodizing oxidizes a metal anode to yield a porous metal oxide coating that can incorporate dye molecules to give brilliant colors. In the oxidation of aluminum, for instance, the electrode reactions are The thickness of the aluminum oxide coating that forms on the anode can be controlled by varying the current flow during the electrolysis. How many minutes are required to produce a 0.0100-mm thick coating of Al2O3 (density 3.97 g/cm^3) on a square piece of aluminum metal 10.0 cm on an edge if the current passed through the piece is 0.600 A?

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Textbook Question

In order to charge a lead storage battery (Section 19.10) 500.0 g of PbSO4(s) must be converted into PbO2(s) and Pb(s). (a) Does the reaction represent an electrolytic or galvanic cell?

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Consider the following half-reactions and E° values: (c) Write the cell reaction for part (b), and calculate the values of E°, ∆G° (in kilojoules), and K for this reaction at 25 °C

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Textbook Question

A concentration cell has the same half-reactions at the anode and cathode, but a voltage results from different concentrations in the two electrode compartments. (b) A similar cell has 0.10 M Cu2+ in both compartments. When a stoichiometric amount of ethylenediamine (NH2CH2CH2NH2) is added to one compartment, the measured cell potential is 0.179 V. Calculate the formation constant Kf for the complex ion Cu(NH2CH2CH2CH2)22+. Assume there is no volume change.

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Textbook Question

Consider a galvanic cell that utilizes the following half-reactions:

(b) What are the values of E° and the equilibrium constant K for the cell reaction at 25 °C?

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Textbook Question

The nickel–iron battery has an iron anode, an NiO(OH) cathode, and a KOH electrolyte. This battery uses the follow-ing half-reactions and has an E° value of 1.37 V at 25 °C. (b) Calculate ∆G° (in kilojoules) and the equilibrium con-stant K for the cell reaction at 25 °C.

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Textbook Question

Experimental solid-oxide fuel cells that use butane (C4H10) as the fuel have been reported recently. These cells contain composite metal/metal oxide electrodes and a solid metal oxide electrolyte. The cell half-reactions are (c) How many grams of butane are required to produce a constant current of 10.5 A for 8.00 h? How many liters of gaseous butane at 20 °C and 815 mm Hg pressure are required?

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Textbook Question

Experimental solid-oxide fuel cells that use butane (C4H10) as the fuel have been reported recently. These cells contain composite metal/metal oxide electrodes and a solid metal oxide electrolyte. The cell half-reactions are (b) Use the thermodynamic data in Appendix B to calculate the values of E° and the equilibrium constant K for the cell reaction at 25 °C. Will E° and K increase, decrease, or remain the same on raising the temperature?

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Textbook Question

The half-reactions that occur in ordinary alkaline batteries can be written as In 1999, researchers in Israel reported a new type of alkaline battery, called a 'super-iron' battery. This battery uses the same anode reaction as an ordinary alkaline battery but involves the reduction of FeO42- ion (from K2FeO4) to solid Fe(OH)3 at the cathode. (a) Use the following standard reduction potential and any data from Appendixes C and D to calculate the stan-dard cell potential expected for an ordinary alkaline battery:

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Textbook Question

Gold metal is extracted from its ore by treating the crushed rock with an aerated cyanide solution. The unbalanced equation for the reaction is (b) Use any of the following data at 25 °C to calculate ∆G° for this reaction at 25 °C: Kf for Au(CN)2- = 6.2 x 10^38, Ka for HCN = 4.9 x 10^-10, and standard reduction potentials are

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Textbook Question

Consider the redox titration of 100.0 mL of a solution of 0.010 M Fe2+ in 1.50 M H2SO4 with a 0.010 M solution of KMnO4, yielding Fe3+ and Mn2+. The titration is carried out in an electrochemical cell equipped with a platinum electrode and a calomel reference electrode consisting of an Hg2Cl2/Hg electrode in contract with a saturated KCl solution having [Cl-] = 2.9M. Using any data in Appendixes C and D, calculate the cell potential after addition of (a) 5.0 mL, (b) 10.0mL, (c) 19.0 mL, and (d) 21.0 mL of the KMnO4 solution.

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A substance with the potential to cause reduction in another substance is __________.

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A substance with the potential to cause oxidation in another substance is __________.

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Which of the following is true about a redox reaction? In a redox reaction, the reducing agent loses electrons. In a redox reaction, the oxidizing agent loses electrons. In a redox reaction, the oxidized species gains electrons. In a redox reaction, the reduced species loses electrons.

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Identify the oxidizing agent and the reducing agent for 4Li(s) + O₂(g) → 2Li₂O(s)

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Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.) 3 Cl₂(g) + 2 Fe(s) → 6 Cl^-(aq) + 2 Fe³⁺(aq) Cl₂(g) + 2 e^- → 2 Cl^-(aq) E° = +1.36 V Fe³⁺(aq) + 3 e^- → Fe(s) E° = -0.04 V

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What element is being reduced in the following redox reaction? Cr(OH)₄^-(aq) + ClO^-(aq) → CrO₄^2-(aq) + Cl^-(aq)

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Which element is oxidized in this reaction? Fe₂O₃ + 3CO → 2Fe + 3CO₂

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Which element is reduced in this reaction? 2KMnO₄ + 3Na₂SO₃ + H₂O → 2MnO₂ + 3Na₂SO₄ + 2KOH

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Which substance is the oxidizing agent in this reaction? 2CuO + C → 2Cu + CO₂

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A chemical reaction that has the general formula of AB → A + B is best classified as what type of reaction?

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Which of the following reactions are redox reactions?

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Oxidation is the ________, and reduction is the ________.

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Which of the following reactions would be classified as oxidation-reduction?

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Which of the following statements is true about the reaction between zinc and copper sulfate?

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Identify the oxidizing agent and the reducing agent for each reaction:

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Identify the oxidizing agent and the reducing agent for 4Li(s) + O₂(g) → 2Li₂O(s).

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Which of the following is true about a redox reaction? In a redox reaction, the reducing agent loses electrons. In a redox reaction, the oxidizing agent loses electrons. In a redox reaction, the oxidized species gains electrons. In a redox reaction, the reduced species loses electrons.

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Determine E° (cell) for the reaction Al(s) + 3 Ag⁺(aq) → 3 Ag(s) + Al³⁺(aq).

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What is E° (cell) for the reaction 2 Au(s) + 3 Ca²⁺(aq) → 2 Au³⁺(aq) + 3 Ca(s)?

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______________________ accelerates the rusting process.

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The presence of which reactant is the best indicator of an oxidation-reduction reaction?

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What species is/are formed at the anode of the alkaline fuel cell?

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in a reaction, a molecule loses an electron. this is an example of which type of reaction?

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What is the standard cell potential for the reaction 2 Cr + 3 Pb²⁺ → 3 Pb + 2 Cr³⁺?

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Use the information in the aleks data tab to sort the following chemical species by reducing power.

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Cl₂(g)+ 2 F⁻(aq) → F₂(g) + 2 Cl⁻(aq)

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What is the balanced reaction for the cell diagram below? Al(s) | Al³⁺(aq) || Cd²⁺(aq) | Cd(s)

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Which element is oxidized in this reaction? ZNO + C --> ZN + CO

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For the following electrochemical cell

Cu(s) | Cu₂(aq, 0.0155 m) || Ag(aq, 2.50 m) | Ag(s)

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H₂(g) + F₂(g) → 2 H⁺(aq) + 2 F⁻(aq).

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Consider the following reaction and select the false statement below. NaI + 3 HOCl → NaIO₃ + 3 HCl

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Which of the following metals would act as a sacrificial anode (cathodic protection) for iron

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Which type of reaction has the general formula of AB + CD → AD + CB?

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What is it called when a substance loses an electron and oxygen is acquired?

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In redox reactions, the reactant that is oxidized is also called the _________.

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Separate this redox reaction into its balanced component half-reactions. Cl₂ + 2K

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Oxidation involves the ________, and reduction involves the

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In the reaction shown below, which substance is oxidized? 2 Cr(s) + Fe₂O₃(aq) → Cr₂O₃(aq) + 2 Fe(s)

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When a(n) _________ agent oxidizes, it causes reduction in another substance.

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