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Question
Nernst equation for the following cell reaction at 298 K is:
\[\ce{Mg_{(s)} | Mg^{2+}_{( aq)} || Ag^+_{( aq)} | Ag_{(s)}}\]
Options
Ecell = `"E"_"cell"^0 - 0.0592/2 log_10 (["Mg"^(2+)])/(["Ag"^+])`
Ecell = `"E"_"cell"^0 - 0.0592/3 log_10 (["Mg"^(2+)])/(["Ag"^+]^2)`
Ecell = `"E"_"cell"^0 - 0.0592/2 log_10 (["Mg"^(2+)])/(["Ag"^+]^2)`
Ecell = `"E"_"cell"^0 - 0.0592 log_10 (["Mg"^(2+)])/(["Ag"^+]^2)`
MCQ
Solution
Ecell = `"E"_"cell"^0 - 0.0592/2 log_10 (["Mg"^(2+)])/(["Ag"^+]^2)`
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Electrode Potential and Cell Potential
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