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Calculate the values of and for the following cell reaction at : (Given: ; , , ) Calculate how long…
(a)[2.0]
Calculate the values of $E_{\text{cell}}$ and $\Delta G$ for the following cell reaction at $25^\circ\text{C}$:
$\text{Zn(s)} / \text{Zn}^{2+}(0\cdot0004\text{M}) \parallel \text{Cd}^{2+}(0\cdot2\text{M}) / \text{Cd(s)}$
(Given: $E^\circ(\text{Zn}^{2+}/\text{Zn}) = -0\cdot763\text{ V}$; $E^\circ(\text{Cd}^{2+}/\text{Cd}) = -0\cdot403\text{ V}$, $1\text{ Faraday} = 96,500\text{ coulombs}$, $R = 8\cdot314\text{ J K}^{-1}\text{ mol}^{-1}$)
(b)[1.0]
Calculate how long it will take to deposit $1\cdot0\text{ g}$ of chromium when a current of $1\cdot25\text{ ampere}$ flows through a solution of chromium (III) sulphate.
(Atomic weight of $\text{Cr} = 52$, $1\text{ Faraday} = 96,500\text{ coulombs}$.)
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From ISC 2026 Specimen Chemistry Paper 1, question 16(ii).