Given below are two statements: Given: Molar mass of C, H, O, Cl...

Statement I:
$30\%$ (w/w) solution of methanol in CCl$_4$ means $30$ g of methanol is present in $70$ g of CCl$_4$.

Molar mass of methanol (CH$_3$OH) $= 12 + 4 \times 1 + 16 = 32$ g mol$^{-1}$
Molar mass of CCl$_4 = 12 + 4 \times 35.5 = 154$ g mol$^{-1}$

Moles of methanol $= \dfrac{30}{32} = 0.9375$ mol
Moles of CCl$_4 = \dfrac{70}{154} = 0.4545$ mol

Mole fraction of CCl$_4 = \dfrac{0.4545}{0.9375 + 0.4545} = \dfrac{0.4545}{1.392} \approx 0.326 \approx 0.33$
Thus, Statement I is true.

Statement II:
In pure methanol, molecules are held together by strong intermolecular hydrogen bonding. On adding CCl$_4$, its molecules come between methanol molecules and break the hydrogen bonds. This decreases the intermolecular attractive forces, leading to an increase in vapour pressure. Hence, the mixture shows a positive deviation from Raoult's law.
Thus, Statement II is true.

Both Statement I and Statement II are true.

Answer: Both Statement I and Statement II are true