The standard EMF for the cell reaction: is 1.10 volts at 25°C. The EMF of the cell reaction when 0.1 — Electrochemistry Chemistry Question
Question
The standard EMF for the cell reaction: $Zn(s) + Cu^{2+}(aq) \rightarrow Zn^{2+}(aq) + Cu(s)$ is 1.10 volts at 25°C. The EMF of the cell reaction when 0.1 M Cu$^{2+}$ and 0.1 M Zn$^{2+}$ solutions are used at 25°C is
Answer: A
💡 Solution & Explanation
According to the Nernst equation: $E_{cell} = E^\circ_{cell} - \frac{0.0591}{2} \log \frac{[Zn^{2+}]}{[Cu^{2+}]}$. When both concentrations are 0.1 M, their ratio is 1, and $\log(1) = 0$. Thus, $E_{cell} = E^\circ_{cell} = 1.10$ V. Therefore, correct answer is A.
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