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Question
Write the Nernst equation and emf of the following cell at 298 K:
\[\ce{Sn_{(s)} | Sn^{2+} (0.050 M) || H^+ (0.020 M) | H2_{(g)} (1 bar) | Pt_{(s)}}\]
Solution
The cell reaction is as follows:
\[\ce{Sn_{(s)} + 2H^+ (0.020 M) -> Sn^{2+} (0.050 M) + H2 (1 bar)}\]
Hence n = 2,
According to this, the Nernst equation will be as follows:
`"E"_"cell" = ("E"_("H"^+//1/2"H"_2)^Θ - "E"_("Sn"^(2+)//"Sn")^Θ) - 0.059/2 log_10 (["Sn"^(2+)] xx "pH"_2)/(["H"^+]^2)`
∴ `"E"_"cell" = [0 - (-0.14)] - 0.059/2 log_10 (0.050 xx 1)/(0.020)^2`
= `0.14 - 0.059/2 log_10 125`
= 0.078 V
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