- A$FeC_2O_4$
- ✓$Fe_2(C_2O_4)_3$
- C$K_4Fe(CN)_6$
- D$FeSO_4$
$Cr_2O_7^{2-} +2OH^- \to 2CrO_4^{2-} +H_2O$
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A $4.0$ molar aqueous solution of $\mathrm{NaCl}$ is prepared and $500 \mathrm{~mL}$ of this solution is electrolysed. This leads to the evolution of chlorine gas at one of the electrodes (atomic mass: $\mathrm{Na}=23, \mathrm{Hg}=200 ; 1$ Faraday $=96500$ coulombs)
$1.$ The total number of moles of chlorine gas evolved is
$(A)$ $0.5$ $(B)$ $1.0$ $(C)$ $2.0$ $(D)$ $3.0$
$2.$ If the cathode is a $\mathrm{Hg}$ electrode, the maximum weight ( $\mathrm{g}$ ) of amalgam formed from this solution is
$(A)$ $200$ $(B)$ $225$ $(C)$ $400$ $(D)$ $446$
$3.$ The total charge (coulombs) required for complete electrolysis is
$(A)$ $24125$ $(B)$ $48250$ $(C)$ $96500$ $(D)$ $193000$
Give the answer question $1,2$ and $3.$

$6 \mathrm{OH}^{-}+\mathrm{Cl}^{-} \rightarrow \mathrm{ClO}_{3}^{-}+3 \mathrm{H}_{2} \mathrm{O}+6 \mathrm{e}^{-}$
A current of $x A$ has to be passed for $10 h$ to produce $10.0 \mathrm{~g}$ of potassium chlorate. The value of $\mathrm{x}$ is $.......$ (Nearest integer)
(Molar mass of $\left.\mathrm{KClO}_{3}=122.6 \mathrm{~g} \mathrm{~mol}^{-1}, \mathrm{~F}=96500 \mathrm{C}\right)$