0.6 g of a solute is dissolved in 0.1 litre of a solvent which develops an osmotic pressure of 1.23 atm at 27°C. The molecular mass of the substance is

Question

0.6 g of a solute is dissolved in 0.1 litre of a solvent which develops an osmotic pressure of 1.23 atm at 27°C. The molecular mass of the substance is (A) 149.5 g mol-1 (B) 120 g mol-1 (C) 430 g mol-1 (D) None of these

Tardigrade Admin · Accepted Answer

m=(wRT/PV) =(0.6×0.082×300/1.23×0.1)=120

Q. 0.6 g of a solute is dissolved in 0.1 litre of a solvent which develops an osmotic pressure of 1.23 atm at $2 7^{\circ} C$ . The molecular mass of the substance is

$149.5 g m o l^{- 1}$

$120 g m o l^{- 1}$

$430 g m o l^{- 1}$

None of these

$m = \frac{wRT}{P V}$
$= \frac{0.6 \times 0.082 \times 300}{1.23 \times 0.1} = 120$

Q. 0.6 g of a solute is dissolved in 0.1 litre of a solvent which develops an osmotic pressure of 1.23 atm at 27∘C. The molecular mass of the substance is

149.5gmol−1

120gmol−1

430gmol−1