The vapour pressures of chloroform (CHCl_3) a | vedclass

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(B) $1$. Calculate moles of each component: $n_{CHCl_3} = \frac{59.75 \ g}{119.5 \ g \cdot mol^{-1}} = 0.5 \ mol$ $n_{CH_2Cl_2} = \frac{21.25 \ g}{85

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$0.491, 0.509$

Vedclass · Answer

(B) $1$. Calculate moles of each component: $n_{CHCl_3} = \frac{59.75 \ g}{119.5 \ g \cdot mol^{-1}} = 0.5 \ mol$ $n_{CH_2Cl_2} = \frac{21.25 \ g}{85 \ g \cdot mol^{-1}} = 0.25 \ mol$ $2$. Calculate mole fractions in liquid phase: $x_{CHCl_3} = \frac{0.5}{0.5 + 0.25} = \frac{0.5}{0.75} = \frac{2}{3}$ $x_{CH_2Cl_2} = \frac{0.25}{0.5 + 0.25} = \frac{0.25}{0.75} = \frac{1}{3}$ $3$. Calculate partial pressures: $P_{CHCl_3} = x_{CHCl_3} 	imes P^0_{CHCl_3} = \frac{2}{3} 	imes 200 \ mmHg = 133.33 \ mmHg$ $P_{CH_2Cl_2} = x_{CH_2Cl_2} 	imes P^0_{CH_2Cl_2} = \frac{1}{3} 	imes 415 \ mmHg = 138.33 \ mmHg$ $4$. Calculate total pressure: $P_{total} = 133.33 + 138.33 = 271.66 \ mmHg$ $5$. Calculate mole fractions in vapour phase $(y_i = \frac{P_i}{P_{total}})$: $y_{CHCl_3} = \frac{133.33}{271.66} \approx 0.491$ $y_{CH_2Cl_2} = \frac{138.33}{271.66} \approx 0.509$

$100 \times x_{acetone}$	$0, 11.8, 23.4, 36.0, 50.8, 85.2, 64.5, 72.1$
$p_{acetone} / mm \, Hg$	$0, 54.9, 110.1, 202.4, 322.7, 405.9, 454.1, 521.1$
$p_{chloroform} / mm \, Hg$	$632.8, 548.1, 469.4, 359.7, 257.7, 193.6, 161.2, 120.7$

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