A sample of air contains N_2, O_2 and H_2O. I | vedclass

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(D) Total pressure $P_{total} = P_{N_2} + P_{O_2} + P_{H_2O} = 640 \, torr$. Given $P_{H_2O} = 40 \, torr$,so the pressure of dry air is $P_{dry} = P_

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$450$

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(D) Total pressure $P_{total} = P_{N_2} + P_{O_2} + P_{H_2O} = 640 \, torr$. Given $P_{H_2O} = 40 \, torr$,so the pressure of dry air is $P_{dry} = P_{N_2} + P_{O_2} = 640 - 40 = 600 \, torr$. Since partial pressure is proportional to the mole fraction,the ratio of partial pressures $P_{N_2} : P_{O_2}$ is equal to the molar ratio $3:1$. Let $P_{N_2} = 3x$ and $P_{O_2} = x$. $3x + x = 600 \implies 4x = 600 \implies x = 150 \, torr$. Therefore,$P_{N_2} = 3 	imes 150 = 450 \, torr$.

$A$ sample of air contains $N_2, O_2$ and $H_2O$. It is saturated with water vapor and the total pressure is $640 \, torr$. The vapor pressure of water is $40 \, torr$ and the molar ratio of gases ${N_2}:{O_2}$ is $3:1$. What is the partial pressure of $N_2$ in the sample in $torr$?

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