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In a cell, the following reactions take place
\[
\begin{array}{l}
\mathrm{Fe}^{2+} \rightarrow \mathrm{Fe}^{3+} \mathrm{f}^{-}, E_{\mathrm{Fe}^{3+} / \mathrm{Fe}^{2+}}^{0}=0.77 \mathrm{~V} \\
2 \mathrm{I}^{-} \rightarrow \mathrm{I}_{2}+2 e^{-}, E_{\mathrm{I}_{2} \mathrm{I}^{-}}^{0}=0.54 \mathrm{~V}
\end{array}
\]
The standard electrode potential for the spontaneous reaction in the cell is \( x \times 10^{-2} V 298 K \). The value of \( x \) is (Nearest Integer)
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