Statement 1 : A solution of Ni(NO₃)₂ is electrolysed between platinum electrodes using current of 5 A for 20 minute. The weight of Ni deposited is 1.825 g.
Statement 2 : The mass of substance deposited during the electrolysis of an electrolyte is inversely proportional to the quantity of electricity passed through the electrolyte.
 

Electricity used  = 5 x 20 x 60 =.6000 C
$\mathrm{Ni}{\left({\mathrm{NO}}_3\right)}_2+2{\mathrm{H}}^{+}+\underset{2\mathrm{F}}{2{\mathrm{e}}^{-}}\to \underset{58.7 \mathrm{g}}{\mathrm{Ni}}+2{\mathrm{HNO}}_3$
Charge required to deposit 1 mole
     Ni = 2 F = 2 x 96500 = 1.93 x 10⁵ C
1.93 x 10⁵ C of charge produce Ni = 58.7 g
$6000 \mathrm{C} \mathrm{charge} \mathrm{will} \mathrm{produce} \mathrm{Ni}=\frac{58.7\times 6000 \mathrm{C}}{1.93\times {10}^5}=1.825 \mathrm{g}$
Assertion is true but reason is false as mass of substance deposited is directly proportional to the quantity of electricity passed.