AP QUIZZES - AP TOPIC 16 Electrochemistry SET C
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QUESTION 1. A REDOX reaction has an Ecell value of +0.81V and involves the transfer of two electrons. Calculate K (the equilibrium constant) for the reaction at 44oC.

(A) 5.8 x 1025
(B) 1.8 x 1025
(C) 2.8 x 1025
(D) 8.5 x 1025
(E) 5.6 x 1025

QUESTION 2. When group I metal salts in solution are electrolyzed, hydrogen gas is produced at the cathode, rather than the free metal. This is because;

(A) Aqueous solutions of group I metals do not conduct electricity
(B) Group I metal salts are insoluble
(C) Water is more easily reduced than group I metal ions in solution
(D) The voltage required for the reaction is too high
(E) None of the above

QUESTION 3. It is possible to extract many metals via the electrolysis of aqueous solutions of their ions. Such an experiment is carried out by passing 3.00 Amps, for 2.00 hours, through a solution of metal ions that carry a 2+ charge. 7.11 grams of the metal was produced. Identify the metal.

(A) Ba
(B) Cu
(C) Ni
(D) Sr
(E) Zn

QUESTION 4. How long would it take in minutes, to produce 5.60 g of Zinc metal from a solution of zinc nitrate using a current of 2.00 Amps?

(A) 138
(B) 826
(C) 65.4
(D) 6.54
(E) 2.00

QUESTION 5. How many electrons are being transferred in the reaction below?

MnO4- + Fe + 2H2O ==> Fe3+ + MnO2 + 4OH-


(A) 0
(B) 1
(C) 2
(D) 3
(E) 4




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