An electrochemical cell at 298 K is made using a copper metal electrode immersed

Question

An electrochemical cell at 298 K is made using a copper metal electrode immersed in a 0.30 M copper sulfate solution in one compartment and a copper metal electrode immersed in a 1.5 M copper sulfate solution in the other compartment. Cu2+(aq) + 2 e- ---> Cu(s), E = +0.34 V Which statement regarding this electrochemical cell is NOT correct? a. The reaction continues until the copper ion concentrations in the two cells are equal. b. The initial cell potential = 0.02 V. c. The cell potential gradually decreases to 0.0 V. d. The standard cell potential is +0.34 V. e. Reduction occurs in compartment C2.

Explanation / Answer

Given:

T = 298 K

First compartment,

[CuSO4]=0.30 M

Second compartment ,

[CuSO4]=1.5 M

Reaction,

Cu2+ + 2e -- > Cu(s)    E=+0.34 V

We know electrode is same and so when we calculate standard electrode potential we use following formula

E0cell= Ecathode – Eanode

Standard reduction potential of the cell is 0.34 V

Lets plug the value in above formula

E0cell =[0.34 – (0.34) ]V

= 0 V

In this case E0 cell = 0 V

So the option d (The standard cell potential is +0.34 V) is incorrect.

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