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(A) $1$. Calculate the moles of acetone $(CH_3COCH_3)$: Molar mass = $58 \ g/mol$. Moles = $174 \ g / 58 \ g/mol = 3 \ mol$.$2$. Calculate the moles o

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$124.8$

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(A) $1$. Calculate the moles of acetone $(CH_3COCH_3)$: Molar mass = $58 \ g/mol$. Moles = $174 \ g / 58 \ g/mol = 3 \ mol$.$2$. Calculate the moles of water $(H_2O)$: Molar mass = $18 \ g/mol$. Moles = $126 \ g / 18 \ g/mol = 7 \ mol$.$3$. Calculate the mole fractions: Total moles = $3 + 7 = 10 \ mol$. $X_{acetone} = 3/10 = 0.3$. $X_{H_2O} = 7/10 = 0.7$.$4$. Apply Raoult's Law: $P_{total} = P^0_{acetone} 	imes X_{acetone} + P^0_{H_2O} 	imes X_{H_2O}$.$5$. $P_{total} = (360 \ torr 	imes 0.3) + (24 \ torr 	imes 0.7) = 108 + 16.8 = 124.8 \ torr$.

Assume that acetone and water form an ideal solution. If $174 \ g$ of acetone $(CH_3COCH_3)$ is mixed with $126 \ g$ of $H_2O$,what is the vapour pressure of the solution at $298 \ K$? Given that ${P^0}_{acetone} = 360 \ torr$ and ${P^0}_{H_2O} = 24 \ torr$ at $298 \ K$.

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