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문제 1
Which of the following unbalanced half-reactions is correctly labeled as an oxidation or reduction? (a) NO3- (aq) → NO(g); reduction (b) Zn(s) → Zn2+(aq); reduction (c) ClO3-(aq) → Cl2(g); oxidation (d) Br-(aq) → Br2(l); reduction
문제 2
What is the coefficient on Sn2+ when the following reaction is balanced in acidic solution?
(a) 2 (b) 4 (c) 5 (d) 7
문제 3
Balance the redox reaction in basic solution. What is the coefficient on the hydroxide ion, and on which side of the equation does it appear? (a) 2 OH- in reactants (b) 4 OH- in products (c) 4 OH- in reactants (d) 3 OH- in reactants
- What is the line notation for the galvanic cell?
문제 5
(a)
(b) (c) (d) - Consider the following table of standard reduction potentials:. Which substance(s) can be reduced by C-? (a) D and B (b) A- (c) D3+ and B2+ (d) A
문제 7
- Calculate E° for each of the following reactions, and determine which are spontaneous under standard-state conditions. (b)
문제 9
- 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.)
문제 10
(a) 8.0 (b) 4.5 (c) 2.2 (d) 3.0 - 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. (a) What are the half-reactions and overall reaction in the battery? (b) Draw a diagram using beakers, a voltmeter, and salt bridge to show how a battery can be constructed. Label the anode, cathode, and direction of electron flow.
문제 12
- 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)
문제 14
- Chlorine can be prepared in the laboratory by the reaction of hydrochloric acid and potassium permanganate. (c) How many liters of Cl₂ at 1.0 atm and 25 °C will result from the reaction of 179 g KMnO₄ with an excess of HCl?
문제 15
문제 19.68
The silver oxide–zinc battery used in watches delivers a voltage of 1.60 V. Calculate the free-energy change (in kilo-joules) for the cell reaction
문제 19.88
Calculate the standard cell potential and the standard free-energy change (in kilojoules) for the reaction below. (See Appendix D for standard reduction potentials.) <QUESTION REFERENCES APPENDIX D>
문제 19.67
How are standard reduction potentials defined?
- Consider a Daniell cell with 1.0 M ion concentrations:
문제 37
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.
- Sketch a cell with inert electrodes suitable for electrolysis of aqueous CuBr2. (b) Indicate the direction of electron and ion flow.
문제 38
문제 40a
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.
(a) Label the anode and cathode, and indicate the signs of the electrodes.
문제 40c
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.
문제 42b
Classify each of the following unbalanced half-reactions as either an oxidation or a reduction. (b) Pt2+ (aq) → Pt(s)
문제 42c
Classify each of the following unbalanced half-reactions as either an oxidation or a reduction. (c) Cr(s) → Cr3+ (aq)
문제 43a
Classify each of the following unbalanced half-reactions as either an oxidation or a reduction. (a) O2(g) → OH-(aq)
문제 43b
Classify each of the following unbalanced half-reactions as either an oxidation or a reduction. (b) H2O2(aq) → O2(g)
문제 43c
Classify each of the following unbalanced half-reactions as either an oxidation or a reduction. (c) MnO4-(aq) → MnO42-(aq)
문제 43d
Classify each of the following unbalanced half-reactions as either an oxidation or a reduction. (d) CH3O→H(aq) CH2O(aq)
문제 44
Balance the half-reactions in Problem 19.42, assuming that they occur in acidic solution.
문제 45
Balance the half-reactions in Problem 19.43, assuming that they occur in basic solution.
문제 46a
Write unbalanced oxidation and reduction half-reactions for the following processes. . (a) Te(s) + NO3-(aq) → TeO2(s) + NO(g)
문제 46b
Write unbalanced oxidation and reduction half-reactions for the following processes. . (b) H2O2(aq) + Fe2+(aq) → Fe3+(aq) + H2O(l)
문제 47a
Write unbalanced oxidation and reduction half-reactions for the following processes. (a) Mn(s) + NO3-(aq) → Mn2+(aq) + NO2(g)
문제 47b
Write unbalanced oxidation and reduction half-reactions for the following processes. (b) Mn3+(aq) → MnO2(s) + Mn2+(aq)
문제 48a
Balance the following half-reactions. (a) (acidic) Cr2O72-(aq) → Cr3+(aq)