\( \text{Cu(s)} + \text{Sn}^{2+}(0.001 \, \text{M}) \longrightarrow \text{Cu}^{2+}(0.01 \, \text{M}) + \text{Sn(s)} \)
The Gibbs free energy change for the above reaction at \( 298 \, \text{K} \) is \( x \times 10^{-1} \, \text{kJ mol}^{-1} \).
The value of \( x \) is ________. [Nearest integer]
[Given: \( E^\ominus_{\text{Cu}^{2+}/\text{Cu}} = 0.34 \, \text{V} \); \( E^\ominus_{\text{Sn}^{2+}/\text{Sn}} = -0.14 \, \text{V} \); \( F = 96500 \, \text{C mol}^{-1} \)]
