For the following cell , `Zn_(s)|ZnSO_(4)((aq)) CuSO_(4)((aq)) |Cu(s)` When the concentration of `Zn^(2+)` is 10 times the concentration of `Cu^(2+)`, the expression for `DeltaG ("in " J mol^(-1)` is [F is Faraday constant , R is gas constant , T is temperature , `E_(cell)^(@) = 1.1V`]

Options

A. (2.30RT-2.2F)
B. (-2.2F)
C. (2.30RT+ 1.1F)`
D. 1.1F

Explanation

To solve the problem, we need to find the expression for \(\Delta G\) in terms of \(F\), \(R\), and \(T\) for the given electrochemical cell reaction. The cell is represented as:

\[ \text{Zn}_{(s)} | \text{ZnSO}_4_{(aq)} \, \text{CuSO}_4_{(aq)} | \text{Cu}_{(s)} \]

Given that the concentration of \(\text{Zn}^{2+}\) is 10 times that of \(\text{Cu}^{2+}\), we can denote the concentration of \(\text{Cu}^{2+}\) as \(C\) and that of \(\text{Zn}^{2+}\) as \(10C\).

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