Equal masses of glucose,sucrose,and urea are | vedclass

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(D) The osmotic pressure $\pi$ is given by the formula $\pi = CRT = (n/V)RT$,where $n$ is the number of moles,$V$ is the volume,$R$ is the gas constan

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$\pi_3 > \pi_1 > \pi_2$

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(D) The osmotic pressure $\pi$ is given by the formula $\pi = CRT = (n/V)RT$,where $n$ is the number of moles,$V$ is the volume,$R$ is the gas constant,and $T$ is the temperature.Since $V, R$,and $T$ are constant for all solutions,$\pi \propto n$.The number of moles $n = 	ext{mass} / 	ext{molar mass}$.Given that the mass is equal for all,$\pi \propto 1 / 	ext{molar mass}$.The molar masses are: Glucose $(C_6H_{12}O_6)$ = $180 \ g/mol$,Sucrose $(C_{12}H_{22}O_{11})$ = $342 \ g/mol$,and Urea $(NH_2CONH_2)$ = $60 \ g/mol$.Since the molar mass of Urea  \pi_1 > \pi_2$.

Equal masses of glucose,sucrose,and urea are dissolved in $V \ L$ of water to prepare separate solutions. The order of osmotic pressures $\pi_1, \pi_2$,and $\pi_3$ for glucose,sucrose,and urea respectively will be...........

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