Chemistry · 2019
JEE Main · 8 April 2019, Shift 2 · Q58
Calculate the standard cell potential (in V) of the cell in which following reaction takes place: Fe^2+( aq )+ Ag^+( aq ) → Fe^3+( aq )+ Ag ( s )…
Calculate the standard cell potential (in V) of the cell in which following reaction takes place :
$$\mathrm{Fe}^{2+}(\mathrm{aq})+\mathrm{Ag}^{+}(\mathrm{aq}) \rightarrow \mathrm{Fe}^{3+}(\mathrm{aq})+\mathrm{Ag}(\mathrm{~s})
$$
Given that
$$\begin{aligned}
& \mathrm{E}_{\mathrm{Ag}^{+} / \mathrm{Ag}}^{\mathrm{o}}=x \mathrm{~V} \\
& \mathrm{E}_{\mathrm{Fe}^{2+} / \mathrm{Fe}}^{\mathrm{o}}=y \mathrm{~V} \\
& \mathrm{E}_{\mathrm{Fe}^{3+} / \mathrm{Fe}}^{\mathrm{o}}=z \mathrm{~V}
\end{aligned}
$$
Official answer
(4)
$\displaystyle x+2 y-3 z$
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JEE Main 2019 Chemistry question, with the answer from NTA’s final answer key. Where our answers come from.