The Gibbs energy change (in J) for the given reaction at [Cu²?] = [Sn²?] = 1M and 298 K is Cu(s) + Sn²?(aq) → Cu²?(aq) + Sn(s); (E?Sn²?/Sn = -0.16V, E?Cu²?/Cu = 0.34 V)
Take F = 96500 Cmol?¹
The Gibbs energy change (in J) for the given reaction at [Cu²?] = [Sn²?] = 1M and 298 K is Cu(s) + Sn²?(aq) → Cu²?(aq) + Sn(s); (E?Sn²?/Sn = -0.16V, E?Cu²?/Cu = 0.34 V)
Take F = 96500 Cmol?¹
Asked by Shiksha User
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1 Answer
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Sol. E? cell = E? (Sn²? |Sn) - E? (Cu²? |Cu)
= -0.16 - 0.34 = -0.50V
ΔG? = -nFE? cell
= -2 × 96500 × (-0.5) = 96500 J
= 96.5 kJ = 96500 J
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