The standard electrode potential `E^(@)` and its temperature coefficient `((dE^(@))/(dT))` for a cell are 2V and `-5xx10^(-4) Vk^(-1)` at 300K respectively . The cell reaction is ` Zn(s)+ Cu^(2) (aq)+ Cu(S)` .
The standard reaction enthalpy `Delta_(r) H^(@)` at 300 K `KJmol^(-1)` is :
`([use R = 8 JK^(-1)mol^(-1)` and `F = 96000Cmol^(-1)])`

Options

A. `206.4`
B. `-412.8`
C. `-384.0`
D. `192.0`

Explanation

To solve the problem, we need to determine the standard reaction enthalpy \(\Delta_r H^\circ\) at 300 K for the given cell reaction:

\[ \text{Zn}(s) + \text{Cu}^{2+}(aq) \rightarrow \text{Zn}^{2+}(aq) + \text{Cu}(s) \]

### Step-by-Step Solution:

1. **Identify the Given Values:**
- Standard electrode potential, \(E^\circ = 2 \, \text{V}\)
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