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

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$0.2$

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(B) The formula for osmotic pressure is $\pi = CRT$. First,calculate the number of moles of solute: $n = \frac{	ext{mass}}{	ext{molar mass}} = \frac{0.822 \ g}{340 \ g \ mol^{-1}} \approx 0.0024176 \ mol$. Next,calculate the molar concentration $C$ in $mol \ L^{-1}$: $C = \frac{n}{V(L)} = \frac{0.0024176 \ mol}{0.300 \ L} \approx 0.0080588 \ M$. Now,substitute the values into the osmotic pressure equation: $\pi = 0.0080588 \ mol \ L^{-1} 	imes 0.0821 \ L \ atm \ mol^{-1} \ K^{-1} 	imes 300 \ K$. $\pi \approx 0.1985 \ atm \approx 0.2 \ atm$.

Calculate the osmotic pressure exerted by a solution containing $0.822 \ g$ of solute in $300 \ mL$ of water at $300 \ K$. (Molar mass of solute $= 340 \ g \ mol^{-1}, R = 0.0821 \ L \ atm \ mol^{-1} \ K^{-1}$) (in $atm$)

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