Write the Nernst equation and calculate the emf of the following cell at 298K. Given: ,
Write the Nernst equation and calculate the emf of the following cell at 298K.
$\text{Mg}(s) \mid \text{Mg}^{2+}(1\times 10^{-3}\text{M}) \parallel \text{Cu}^{2+}(1\times 10^{-4}\text{M}) \mid \text{Cu}(s)$
Given: $E^\circ(\text{Mg}^{2+}/\text{Mg}) = -2\cdot373\text{ V}$, $E^\circ(\text{Cu}^{2+}/\text{Cu}) = +0\cdot337\text{ V}$
Answer
Answer
AIWritten by AI (gemini) - it can contain mistakes.
Nernst equation:
$E_{\text{cell}} = E^\circ_{\text{cell}} - \frac{0\cdot059}{n} \log \frac{[\text{Mg}^{2+}]}{[\text{Cu}^{2+}]}$
$E^\circ_{\text{cell}} = E^\circ_{\text{cathode}} - E^\circ_{\text{anode}} = 0\cdot337 - (-2\cdot373) = +2\cdot71\text{ V}$
Here $n = 2$:
$E_{\text{cell}} = 2\cdot71 - \frac{0\cdot059}{2} \log \frac{1\times 10^{-3}}{1\times 10^{-4}} = 2\cdot71 - 0\cdot0295 \log 10 = 2\cdot71 - 0\cdot0295 = 2\cdot6805\text{ V}$
Final answer: 2.6805 V
Final answer: 2.6805 V
From ISC 2027 Specimen Chemistry Paper 1, question 8.