AP QUIZZES - AP TOPIC 16 Electrochemistry SET A
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QUESTION 1. If the two half-cells below were combined, what would be the correct chemical equation to represent the spontaneous REDOX process?

Cu2+ + 2e- <====> Cu (+0.34V)
H+ + e- <====> 1/2 H2 (0.00V)


(A) Cu2+ + H+ ==> 1/2 H2 + Cu
(B) Cu2+ + 2H+ ==> H2 + Cu
(C) Cu2+ + 1/2 H2 ==> H+ + Cu
(D) Cu2+ + H2 ==> 2H+ + Cu
(E) Cu + 2H+ ==> H2 + Cu2+

QUESTION 2. If the two half-cells below were combined, what would be the voltage generated by the spontaneous REDOX process?

Cu2+ + 2e- <====> Cu (+0.34V)
H+ + e- <====> 1/2 H2 (0.00V)


(A) +0.34V
(B) -0.34V
(C) 0.00V
(D) +0.68V
(E) -0.68V

QUESTION 3. If the two half-cells below were combined, which cell would undergo reduction?

Cu2+ + 2e- <====> Cu (+0.34V)
H+ + e- <====> 1/2 H2 (0.00V)


(A) Hydrogen half-cell
(B) Neither
(C) Both
(D) Copper half-cell
(E) Not enough information to tell

QUESTION 4. If the two half-cells below were combined, what would be the expected products of the spontaneous chemical reaction?

Zn2+ + 2e- <====> Zn (-0.76V)
H+ + e- <====> 1/2 H2 (0.00V)


(A) H+ and Zn2+
(B) H+ and Zn
(C) Zn and H2
(D) H2 and Zn2+
(E) None of the above

QUESTION 5. Which of the following statements is FALSE?

(A) Oxidation involves a loss of electrons
(B) Reduction involves a gain of electrons
(C) A cell can be used to determine a value of Delta G for a REDOX reaction
(D) A spontaneous REDOX reaction has a positive Ecell voltage
(E) Electrolysis of aqueous potassium chloride will yield potassium metal at the cathode




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