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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 $3.$
| gas | $Ar$ | $Ne$ | $Kr$ | $Xe$ |
| $a /\left( atm \,dm ^{6} \,mol ^{-2}\right)$ | $1.3$ | $0.2$ | $5.1$ | $4.1$ |
| $b /\left(10^{-2} \,dm ^{3}\, mol ^{-1}\right)$ | $3.2$ | $1.7$ | $1.0$ | $5.0$ |
Which gas is expected to have the highest critical temperature?
