If the standard electrode potential for a cell is 2V at 300 K, the equilibrium constant (K) for the reaction `Zn(s) + Cu^(2+) (aq)` at 300 k is approximately : `(R=8JK^(-1) mol^(-1) , F= 96000 mol^(-1))`

Options

A. `e^(-160)`
B. `e^(320)`
C. `e^(160)`
D. `e^(-80)`

Explanation

To find the equilibrium constant (K) for the reaction \( \text{Zn(s)} + \text{Cu}^{2+}(aq) \rightleftharpoons \text{Zn}^{2+}(aq) + \text{Cu(s)} \) at 300 K, we can use the relationship between the standard electrode potential (E°), Gibbs free energy change (ΔG°), and the equilibrium constant (K).

### Step-by-Step Solution:

1. **Identify the Reaction and Variables**:
The reaction is:
\[
\text{Zn(s)} + \text{Cu}^{2+}(aq) \rightleftharpoons \text{Zn}^{2+}(aq) + \text{Cu(s)}
...