
- A

- ✓

- C

- D







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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 $3.$
phenol $\xrightarrow[{reaction}]{{\operatorname{Re} imer - Tiemann}}X\xrightarrow[{(ii)\,{H^ \oplus }}]{{(i)\,NaOH\,conc}}Z$
Product $Z$ is