4AB › Chemistry PYQ › CSIR-NET › December 2014 › Q89Q89 · CSIR-NET Chemistry, December 2014 Paper: CSIR-NET December 2014 · Subject: Physical Chemistry · Chapter: Electrochemistry · Topic: Nernst Cells · 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: A ✓ checked by 4AB · confidence high
Explanation E°cell = 0.15 − (−0.14) = 0.29 V; ln K = nFE°/RT = 2 × 0.29/0.0257 = 22.6.
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