Calculate the molar mass of solute in a solut | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(D) The osmotic pressure formula is given by $\pi V = nRT = \frac{W_2}{M_2} RT$. Rearranging for molar mass $M_2$: $M_2 = \frac{W_2 RT}{\pi V}$. Given

Vedclass · Accepted Answer

$410 \ g \ mol^{-1}$

Vedclass · Answer

(D) The osmotic pressure formula is given by $\pi V = nRT = \frac{W_2}{M_2} RT$. Rearranging for molar mass $M_2$: $M_2 = \frac{W_2 RT}{\pi V}$. Given: $W_2 = 1 \ g$,$V = 0.3 \ dm^3$,$\pi = 0.2 \ atm$,$T = 300 \ K$,$R = 0.082 \ dm^3 \ atm \ K^{-1} \ mol^{-1}$. Substituting the values: $M_2 = \frac{1 \ g 	imes 0.082 \ dm^3 \ atm \ K^{-1} \ mol^{-1} 	imes 300 \ K}{0.2 \ atm 	imes 0.3 \ dm^3}$. $M_2 = \frac{24.6}{0.06} \ g \ mol^{-1} = 410 \ g \ mol^{-1}$.

Calculate the molar mass of solute in a solution prepared by dissolving $1 \ g$ in $0.3 \ dm^3$ solvent having osmotic pressure $0.2 \ atm$ at $300 \ K$. $\left[R=0.082 \ dm^3 \ atm \ K^{-1} \ mol^{-1}\right]$

Similar Questions

What is the osmotic pressure $(\pi)$ of a $0.02 \ M$ solution of $NaCl$ (in $RT$)?

Isotonic solutions have the same

Pickles have a long shelf life and do not get spoiled for months,why?

What is osmotic pressure? Explain and derive its equation.

$A$ $1\% \ (wt/vol) \ KCl$ solution is ionised to the extent of $80\%$. The osmotic pressure at $27 \ ^oC$ of the solution will be .......... $atm$.

Vedclass Test Series

Exam Paper Generator

Online Exam Module