If the standard electrode potential for a cell is 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 \( \text{Zn(s)} + \text{Cu}^{2+}(aq) \rightarrow \text{Zn}^{2+}(aq) + \text{Cu(s)} \) at 300 K, given that the standard electrode potential (\( E^\circ \)) for the cell is 2 V, we can use the relationship between the standard electrode potential and the equilibrium constant.

### Step-by-Step Solution:

1. **Identify the Given Values:**
- Standard electrode potential, \( E^\circ = 2 \, \text{V} \)
- Temperature, \( T = 300 \, \text{K} \)
- Faraday's constant, \( F = 96000 \, \text{C/mol} \)
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