ABC26PH0993 · Electrochemistry

Subject: Physical Chemistry · Chapter: Electrochemistry · Topic: Nernst Cells · Exam: NET DEC 2014 · Marks: 2 · Difficulty: Medium

For the cell reaction, $\mathrm{Sn}(\mathrm{s})+\mathrm{Sn}^{4+}(\mathrm{aq}) 2 \mathrm{Sn}^{2+}(\mathrm{aq})$, separate electrode reactions could be written with the respective standard electrode potential data at 25°C as 4
\[ \mathrm{Sn} 2+(\mathrm{aq})+2 \mathrm{e} \rightarrow \mathrm{Sn}(\mathrm{s}), \quad \mathrm{E}_{\mathrm{o}}=-0.14 \mathrm{V} \]
When RT/F is given as 25.7 mV , logarithm of the equilibrium constant $(\ln \mathrm{K})$ is
(a)22.6
(b)226
(c)2.26
(d)$2.26 \times 10^{-1}$
Answer
Answer (as printed): A
Explanation
No explanation was printed for this question.

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