$Cu(S)+Sn^{2+} (0.001M) Cu^{2+} (0.01M) + Sn(s)$ The Gibbs free energy change for the above reaction at 298 K is x × 10 -1 × kJ mol -1 . The value of x is ________ .[nearest integer] [Given $E^{-}_{cu^{2+} / cu} = 0.34V; E^{-}_{Sn^{2+} / Sn} = - 0.14V; F = 96500 C ∼ mol^{-1}$ ]

Question

$Cu(S)+Sn^{2+} (0.001M) Cu^{2+} (0.01M) + Sn(s)$ The Gibbs free energy change for the above reaction at 298 K is x × 10 -1  × kJ mol -1 . The value of x is ________ .[nearest integer] [Given  $E^{-}_{cu^{2+} / cu} = 0.34V; E^{-}_{Sn^{2+} / Sn} = - 0.14V; F = 96500 C ∼ mol^{-1}$ ]

cdquestions Admin · Accepted Answer

The correct answer is 983 $Cu + Sn^{2+} → Cu^{2+} + Sn(s)$ $E°_{cell} = E°_{Ox} + E°_{Red }$ = -  0.34 - 0.14 = 0.48 V $E = E° - \frac{0.0591}{2} log\frac{[ Cu^{2+}]}{[ Sn^{2+}]}$ = - 0.48 - 0.0295 log 10 = - 0.5095 V $ΔG = -nFE$ = -2 × 96500 × 0.5095 J / mol = 98333.5 × 10 -3 kJ / mol = 983.3 × 10 -1 kJ / mol = 983 × 10 -1 kJ / mol

\(Cu(S)+Sn^{2+} (0.001M) Cu^{2+} (0.01M) + Sn(s)\)
The Gibbs free energy change for the above reaction at 298 K is x × 10^-1 × kJ mol^-1. The value of x is ________ .[nearest integer]
[Given \(E^{-}_{cu^{2+} / cu} = 0.34V; E^{-}_{Sn^{2+} / Sn} = - 0.14V; F = 96500 C ∼ mol^{-1}\)]

Correct Answer: 983

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\(Cu(S)+Sn^{2+} (0.001M) Cu^{2+} (0.01M) + Sn(s)\)The Gibbs free energy change for the above reaction at 298 K is x × 10-1 × kJ mol-1. The value of x is ________ .[nearest integer][Given \(E^{-}_{cu^{2+} / cu} = 0.34V; E^{-}_{Sn^{2+} / Sn} = - 0.14V; F = 96500 C ∼ mol^{-1}\)]