Question 1

Which statement best explains why copper(II) ions can oxidize silver metal in a redox reaction?

Accepted Answer

Copper(II) ions have a greater attraction for electrons than silver ions.

Question 2

During the process of photosynthesis, $$6CO_2 + 6H_2O \rightarrow C_6H_{12}O_6$ + 6O_2$$, which element is reduced?

Accepted Answer

Carbon in carbon dioxide.

Question 3

Which of the following solutions should NOT be stored in a tin-plated container?

Accepted Answer

II) $$AgNO_3(aq) $$and IV) $$CuSO_4(aq)$$

Question 4

Which chemical will reduce copper(II) ions and also oxidize metallic nickel?

Accepted Answer

Iron(II) nitrate

Question 5

A high school laboratory’s waste container is used to dispose of aqueous solutions of sodium nitrate, potassium sulfate, hydrochloric acid, and tin(II) chloride. The most likely net redox reaction to occur inside the waste container is:

Accepted Answer

$$2Cr_2O_7$$^{2-}$$_{(aq)} + 14H^+_{(aq)} + 6Sn$$^{2+}$$_{(aq)} \rightarrow 3Sn$$^{4+}$$_{(aq)} + 2Cr$$^{3+}$$_{(aq)} + 7H_2O_{(l)}$$

Question 6

Given the half-reactions: $$SeO_4$$^{2-} + 2e^- \rightarrow $$SeO_3$$^{2-}$$ and Au$$^{3+}$$ + 3e^- \rightarrow Au$$, which species is the oxidizing agent?

Accepted Answer

$$Au^{3+}$$

Question 7

Which of the following redox reactions is spontaneous under standard conditions?

Accepted Answer

$$In^3+ + 3e$$^- \rightarrow In(s)$$ and Li^+ + 3e$$^- \rightarrow Li(s)$$

Question 8

A potassium permanganate solution is added to an acidic iron(II) sulfate solution. Which balanced equation best represents the spontaneous redox reaction?

Accepted Answer

$$MnO_4$$^-_{(aq)} + 8H^+_{(aq)} + $$5Fe^{2+}$$_{(aq)} \rightarrow $$Mn^{2+}$$_{(aq)} + $$5Fe^{3+}$$_{(aq)} + 4H_2O_{(l)}$$

Question 9

Balance the following redox equation using the oxidation number method: $$SO_2 + 2H_2O$$ + $$Br_2$$ \rightarrow 2Br^- + $$SO_4$$^{2-} + 4H^+$$. What is the sum of the coefficients for all species?

Accepted Answer

8

Question 10

A redox titration was completed by titrating 10.0 mL of tin(II) chloride solution with acidified 0.0967 mol/L potassium dichromate. If an average volume of 12.4 mL of potassium dichromate was required, what is the molar concentration of the tin(II) solution?

Accepted Answer

$$0.360\ mol/L$$

Question 11

Which of the following is the correct oxidation half-reaction for $$SeO_3$$^{2-}$$ being converted to $$SeO_4$$^{2-}$$?

Accepted Answer

$$SeO_3$$^{2-} \rightarrow $$SeO_4$$^{2-} + 2e^-$$

Question 12

In a redox reaction, which species acts as the reducing agent?

Accepted Answer

The species that loses electrons.

Question 13

Which of the following statements about spontaneous redox reactions is correct?

Accepted Answer

A spontaneous redox reaction occurs when the standard cell potential $$E^\circ_{cell} is $$positive.

Question 14

If $$n = C 	imes V$$, where $$n is $$the number of moles, $$C is $$concentration in mol/L, and $$V is $$volume in L, what is the number of moles in 0.250 L of a 0.0967 mol/L solution?

Accepted Answer

$$0.0242\ mol$$

Question 15

Which of the following is a correct reduction half-reaction for $$Au^{3+}$$?

Accepted Answer

$$Au^{3+} + 3e$$^- \rightarrow Au$$

Question 16

In a redox titration, why is it important to use an indicator that changes color at the equivalence point?

Accepted Answer

To accurately determine when the reaction is complete.

Question 17

Which of the following best describes the role of potassium dichromate in a redox titration with tin(II) chloride?

Accepted Answer

It acts as the oxidizing agent.

Question 18

In the reaction $$MnO_4$$^-_{(aq)} + 8H^+_{(aq)} + $$5Fe^{2+}$$_{(aq)} \rightarrow $$Mn^{2+}$$_{(aq)} + $$5Fe^{3+}$$_{(aq)} + 4H_2O_{(l)}$$, which species is oxidized?

Accepted Answer

$$Fe^{2+}$$

Redox Reactions and Electrochemistry: Study Notes

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