- AAcetone
- ✓Ethyl alcohol
- CDiethyl ether
- DChloroform
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Product $(A)$ of the above reaction is
$2 \mathrm{Fe}^{3+}(\mathrm{aq})+2 \mathrm{I^-}(\mathrm{aq}) \rightarrow 2 \mathrm{Fe}^{2+}(\mathrm{aq})+\mathrm{I}_{2}(\mathrm{aq})$
$\mathrm{E}_{\text {call }}^{\mathrm{e}}=0.24 \mathrm{V}$ at $298\; \mathrm{K}$. The standard Gibbs energy $\left( {{\Delta _r}{{\rm{G}}^ \ominus }} \right)$ of the cell reaction is:
[Faraday constant $\mathrm{F}=96500 \;\mathrm{C} \mathrm{mol}^{-1} $]
$\mathrm{CO}_2, \mathrm{NO}_2, \mathrm{H}_2 \mathrm{SO}_4, \mathrm{BF}_3, \mathrm{CH}_4, \mathrm{SiF}_4, \mathrm{ClO}_2, \mathrm{PCl}_5,$ $\mathrm{BeF}_2, \mathrm{C}_2 \mathrm{H}_6, \mathrm{CHCl}_3, \mathrm{CBr}_4$
${\log _{10}}K = - \frac{{2000}}{T} + 6.0$ Activation energy is ....... $kcal$
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The compounds $A$ and $B$ respectively are ......