Question

Calculate Standard Gibbs free energy change for the given reaction. Given Standard Electrode Reduction Potential of Copper and Zinc electrode -> 0.34 V and -0.76 V respectively. Cu²+ + Zn ----> Cu+ Zn²+​

Answer 1

Answer:

The standard EMF of the given cell is: Ecell0=ECu2+∣Cu0−EZn2+∣Zn0=0.34V−(−0.76V)=1.1V.

The EMF of cell is: Ecell=Ecell0−n0.059log[Cu2+][Zn2+].

Ecell=1.1V−20.059log0.0050.05=1.1V−0.0295V=1.0705V.

Answer 2

Answer:

Explanation:

⇒ the standard EMF of the given cell is:E ^0 cell=E^0 base cu^2+|Cu-E^0 base Zn^2+|Zn=0.34 V -(-0.76 V)=1.1 V.

⇒the EMF of cell is:E base cell =E^0 base cell -0.059/n log [Zn^2+/Cu^2+].

⇒E base cell=1.1 V -0.059/2 log 0.05/0.005=1.1 V -0,0295 V= 1.0705 V.

∴ 1.0705 V

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