A solution of sucrose (Molar mass = 342 g/mol) is prepared by dissolving 68.4 g of it per litre of solution, what is its osmotic pressure (R = 0.082 L atom K-1 mol-1) at 273 K?

Question

A solution of sucrose (Molar mass = 342 g/mol) is prepared by dissolving 68.4 g of it per litre of solution, what is its osmotic pressure (R = 0.082 L atom K-1 mol-1) at 273 K? (A) 3.92 atm (B) 4.48 atm (C) 5.92 atm (D) 29.4 atm

Tardigrade Admin · Accepted Answer

Osmotic pressure (π)= CRT Here, C = concentration of solution C =( n / V ) ∴ n =( w / m )=( text weight in gram of substance / text Mol. weight of substance ) V =1 litre C =(68.4/342) π=(68.4/342) × 0.082 × 273 =4.48 atm

Q. A solution of sucrose (Molar mass = $342 g / m o l$ ) is prepared by dissolving $68.4 g$ of it per litre of solution, what is its osmotic pressure ( $R = 0.082 L$ atom $K^{- 1}$ $m o l^{- 1}$ ) at $273 K$ ?

3.92 atm

4.48 atm

5.92 atm

29.4 atm

Osmotic pressure $(π) = CRT$
Here, $C =$ concentration of solution
$C = \frac{n}{V}$
$∴ n = \frac{w}{m} = \frac{weight in gram of substance}{Mol. weight of substance}$
$V = 1$ litre
$C = \frac{68.4}{342}$
$π = \frac{68.4}{342} \times 0.082 \times 273$
$= 4.48 a t m$

Q. A solution of sucrose (Molar mass = 342g/mol) is prepared by dissolving 68.4g of it per litre of solution, what is its osmotic pressure (R=0.082L atom K−1 mol−1) at 273K?