16. The EMF of the cell at 298 K is 0.2905 V. The equilibrium constant for the standard cell reactio — Electrochemistry Chemistry Question
Question
16. The EMF of the cell $Zn / Zn^{2+}(0.01 M) // Fe^{2+}(0.001 M) / Fe$ at 298 K is 0.2905 V. The equilibrium constant for the standard cell reaction is:
Answer: A
💡 Solution & Explanation
$E = E^\circ - (0.0591/2) \log(0.01 / 0.001) \implies 0.2905 = E^\circ - 0.02955 \log(10) \implies E^\circ = 0.32 V$. At equilibrium, $E^\circ = (0.0591/n) \log K \implies 0.32 = (0.0591/2) \log K \implies \log K = 0.32 / 0.0295 \implies K = 10^{(0.32/0.0295)}$.
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