Problem: Consider the cell described below:Zn | Zn 2+(1.00 M) ‖ Cu 2+(1.00 M) | CuCalculate the cell potential after the reaction has operated long enough for the [Zn 2+] to have changed by 0.20 mol/L. (Assume T = 25°C.)

FREE Expert Solution

Step 1


Zn2+(aq) + 2 e- Zn(s)                      E° = -0.76 V                E°  oxidation  anode
Cu2+(aq) + 2 e-
 Cu(s)                      E° = 0.34 V                 E°  reduction  cathode


Step 2


E°cell = E°cathode - E°anodeE°cell =0.34 V - (-0.76 V)

cell = 1.10 V


Step 3


Zn2+(aq) + 2 e- Zn(s) 

Cu(s)  → Cu2+(aq) + 2 e-

________________________________

Cu2+ (aq) + Zn (s) Cu (s) + Zn2+ (aq)


n = 2


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Problem Details

Consider the cell described below:

Zn | Zn 2+(1.00 M) ‖ Cu 2+(1.00 M) | Cu

Calculate the cell potential after the reaction has operated long enough for the [Zn 2+] to have changed by 0.20 mol/L. (Assume T = 25°C.)

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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.