Osmotic pressure of a urea solution at 10,^{c | vedclass

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(B) The osmotic pressure formula is $\Pi = CRT = \frac{n}{V} RT$,which implies $\Pi V = nRT$.For the initial state: $\Pi_1 = 500\,mm$,$T_1 = 10 + 273

Vedclass · Accepted Answer

$5$

Vedclass · Answer

(B) The osmotic pressure formula is $\Pi = CRT = \frac{n}{V} RT$,which implies $\Pi V = nRT$.For the initial state: $\Pi_1 = 500\,mm$,$T_1 = 10 + 273 = 283\,K$,and volume is $V_1$.For the final state: $\Pi_2 = 105.3\,mm$,$T_2 = 25 + 273 = 298\,K$,and volume is $V_2$.Since the number of moles of urea $n$ remains constant,we have $\frac{\Pi_1 V_1}{T_1} = \frac{\Pi_2 V_2}{T_2}$.Substituting the values: $\frac{500 	imes V_1}{283} = \frac{105.3 	imes V_2}{298}$.$\frac{V_2}{V_1} = \frac{500 	imes 298}{105.3 	imes 283} \approx \frac{149000}{29799.9} \approx 5$.Therefore,the extent of dilution is $5$ times.

Osmotic pressure of a urea solution at $10\,^{\circ}C$ is $500\,mm$. The osmotic pressure of the solution becomes $105.3\,mm$ when it is diluted and the temperature is raised to $25\,^{\circ}C$. The extent of dilution is .......... times.

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