0.7 cm^3 of compound A (molar mass =70 g mol^-1, density =1.024 g cm^-3 ) is dissolved in 1 dm^3 of water. If the depression in freezing point of…

$\displaystyle 0.7 \mathrm{~cm}^3$ of compound A (molar mass $\displaystyle =70 \mathrm{~g} \mathrm{~mol}^{-1}$, density $\displaystyle =1.024 \mathrm{~g} \mathrm{~cm}^{-3}$ ) is dissolved in $\displaystyle 1 \mathrm{dm}^3$ of water. If the depression in freezing point of water is $\displaystyle 0.02$ °C, the van't Hoff factor for the compound A is \_\_\_\_ $\displaystyle \times 10^{-2}$. (Nearest integer) [Given : $\displaystyle \mathrm{K}_{\mathrm{f}}$ for $\displaystyle \mathrm{H}_2 \mathrm{O}=1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$, Density of $\displaystyle \mathrm{H}_2 \mathrm{O}=1.0 \mathrm{~g} \mathrm{~cm}^{-3}$ ]