The osmotic pressure of a solution containing | vedclass

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(A) The formula for osmotic pressure is $\pi = CRT$. First,calculate the number of moles of cane sugar: $n = \frac{	ext{mass}}{	ext{molar mass}} = \

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$2.40$

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(A) The formula for osmotic pressure is $\pi = CRT$. First,calculate the number of moles of cane sugar: $n = \frac{	ext{mass}}{	ext{molar mass}} = \frac{34.2 \ g}{342 \ g \ mol^{-1}} = 0.1 \ mol$. The concentration $C = \frac{n}{V} = \frac{0.1 \ mol}{1 \ L} = 0.1 \ mol \ L^{-1}$. The temperature $T = 20 + 273 = 293 \ K$. Substituting the values: $\pi = 0.1 \ mol \ L^{-1} 	imes 0.082 \ L \ atm \ K^{-1} \ mol^{-1} 	imes 293 \ K = 2.4026 \ atm \approx 2.40 \ atm$.

The osmotic pressure of a solution containing $34.2 \ g$ of cane sugar (molar mass = $342 \ g \ mol^{-1}$) in $1 \ L$ of solution at $20^{\circ} C$ is
(Given,$R = 0.082 \ L \ atm \ K^{-1} \ mol^{-1}$) (in $atm$)

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The osmotic pressure of a solution containing $34.2 \ g$ of cane sugar (molar mass = $342 \ g \ mol^{-1}$) in $1 \ L$ of solution at $20^{\circ} C$ is (Given,$R = 0.082 \ L \ atm \ K^{-1} \ mol^{-1}$) (in $atm$)