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Question
Write the Nernst equation and emf of the following cell at 298 K:
\[\ce{Fe_{(s)} | Fe^{2+} (0.001 M) || H^+ (1 M) | H2_{(g)} (1 bar) | Pt_{(s)}}\]
Solution
The cell reaction is as follows:
\[\ce{Fe_{(s)} + 2H^+ (1 M) -> Fe^{2+} (0.001 M) + H2 (1 bar)}\]
Hence, n = 2,
The Nernst equation for the emf of this cell will be as follows –
`"E"_"cell" = ("E"_("H"^+//1/2"H"_2)^Θ - "E"_("Fe"^(2+)//"Fe")^Θ) - 0.059/2 log_10 (["Fe"^(2+)] xx "pH"_2)/(["H"^+]^2)`
∴ `"E"_"cell" = [0 - (-0.44)] - 0.059/2 log_10 (0.001 xx 1)/(1)^2`
= `0.44 - 0.059/2 log_10 10^-3`
= `0.44 - 0.059/2 xx (-3)`
= 0.529 V
RELATED QUESTIONS
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Calculate the emf of the following cell at 298 K:
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Calculate the value of \[\ce{E^\circ}\]cell, E cell and ΔG that can be obtained from the following cell at 298 K.
\[\ce{Al/Al^3+ _{(0.01 M)} // Sn^{2+} _{(0.015 M)}/Sn}\]
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Calculate the value of ΔG that can be obtained from the following cell at 298K.
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Write the Nernst equation and emf of the following cell at 298 K:
\[\ce{Sn_{(s)} | Sn^{2+} (0.050 M) || H^+ (0.020 M) | H2_{(g)} (1 bar) | Pt_{(s)}}\]
