MCQ
Oxidation number of $S$ in $N{a_2}S{O_4}$ is
- A$-2$
- B$2$
- C$-6$
- ✓$6$
$2 + x - 2 \times 4 = 0$
$x = + 6$.
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Cell notation : $M \left|\underset{0.01}{ M ^{2+}} \| \underset{0.0001}{ M ^{2+}}\right| M$
.........$V$ value of $E _{ Cell }^{o}$ is $4$ volt (Given $\frac{ RT }{ F }$ in $10=0.06$ )
$\left( i \right)\,2F{e_2}{O_3}\left( s \right) \to 4Fe\left( s \right) + 3{O_2}\left( g \right)$
${\Delta _r}{G^o} = + 1487.0\,kJ\,mo{l^{ - 1}}$
$\left( {ii} \right)\,2CO\left( g \right) + {O_2}(g) \to 2C{O_2}\left( g \right)$
${\Delta _r}{G^o} = - 514.4\,kJ\,mo{l^{ - 1}}$
Free energy change, $\Delta_rG^o$ for the reaction
$\,2F{e_2}{O_3}\left( s \right) + 6CO\left( g \right) \to 4Fe\left( s \right) + 6C{O_2}\left( g \right)$ will be .....$kJ\, mol^{-1}$