A sample of air contains N_2 and O_2 saturate | vedclass

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(D) According to Dalton's Law of Partial Pressures,the total pressure $P_{total} = P_{N_2} + P_{O_2} + P_{H_2O}$.Given $P_{total} = 640 \ torr$ and $P

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$450$

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(D) According to Dalton's Law of Partial Pressures,the total pressure $P_{total} = P_{N_2} + P_{O_2} + P_{H_2O}$.Given $P_{total} = 640 \ torr$ and $P_{H_2O} = 40 \ torr$.Therefore,the sum of partial pressures of dry gases is $P_{N_2} + P_{O_2} = 640 - 40 = 600 \ torr$.Since the molar ratio of $N_2$ to $O_2$ is $3 : 1$,the partial pressures are proportional to their mole fractions.Let $P_{N_2} = 3x$ and $P_{O_2} = x$.Then $3x + x = 600 \ torr$,which gives $4x = 600 \ torr$,so $x = 150 \ torr$.The partial pressure of $N_2$ is $P_{N_2} = 3x = 3 	imes 150 = 450 \ torr$.

$A$ sample of air contains $N_2$ and $O_2$ saturated with water vapor,with a total pressure of $640 \ torr$. If the water vapor pressure is $40 \ torr$ and the molar ratio of $N_2$ to $O_2$ is $3 : 1$,what is the partial pressure of $N_2$ in the sample in $torr$?

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