The osmotic pressure at 17 ^oC of an aqueous | vedclass

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Question

(A) The formula for osmotic pressure is $\pi = CRT = \frac{n}{V}RT$. Given: Mass of sucrose $(C_{12}H_{22}O_{11})$ = $1.75 \ g$. Molar mass of sucrose

Vedclass · Accepted Answer

$0.8$

Vedclass · Answer

(A) The formula for osmotic pressure is $\pi = CRT = \frac{n}{V}RT$. Given: Mass of sucrose $(C_{12}H_{22}O_{11})$ = $1.75 \ g$. Molar mass of sucrose = $342 \ g/mol$. Number of moles $(n)$ = $\frac{1.75}{342} \approx 0.005117 \ mol$. Volume $(V)$ = $150 \ mL = 0.150 \ L$. Temperature $(T)$ = $17 + 273 = 290 \ K$. Gas constant $(R)$ = $0.0821 \ L \cdot atm \cdot K^{-1} \cdot mol^{-1}$. Substituting the values: $\pi = \frac{0.005117}{0.150} 	imes 0.0821 	imes 290$. $\pi \approx 0.03411 	imes 23.809 \approx 0.812 \ atm$. Rounding to the nearest option,the value is $0.8 \ atm$.

The osmotic pressure at $17 \ ^oC$ of an aqueous solution containing $1.75 \ g$ of sucrose per $150 \ mL$ solution is .......... $atm$.

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