Cu l Cu^2+ (0.265M) ll Zn^2+ (1.23M) l Zn Cu^(2+) + 2e(-) -> Cu Eo = 0.34 V Zn^(

Question

Cu l Cu^2+ (0.265M) ll Zn^2+ (1.23M) l Zn

Cu^(2+) + 2e(-) -> Cu   Eo = 0.34 V

Zn^(2=) + 2e(-) -> Zn    Eo = -0.76 V

Which statements are true?

a. Adding equal amount of water to both halves will not change the potential of the cell

b. Increading the concentration of Cu^2+ will decrease the concentration of the reaction

c. Increasing the concentration of Zn^2+ will decrease the potential of the cell

d. Oxidation takes place at the anode

e. using Pt electrode in place of Cu electrode will not changre the potential of the cell

I'm second-guessing myself here and it's killer.

Explanation / Answer

a)
As the concentrations of Cu+2 and Zn+2 solutions are not same, by adding equal amounts of water to them their concentrations wont be changed by same extent, so, the potentials will be changed.

b) By Increading the concentration of Cu^2+ will decrease the reaction quotient.

c) Yes, Increasing the concentration of Zn^2+ will decrease the potential of the cell.

d) true. Oxidation takes place at the anode

             Zn -----------------> Zn+2 + 2e-

e) False. pt is inert electrode which can be used to transportation of e-s only

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