A sample of O_2 gas is collected over water a | vedclass

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(C) According to Dalton's Law of partial pressures,the total pressure is the sum of the partial pressure of the dry gas and the vapor pressure of wate

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$0.96\,atm$

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(C) According to Dalton's Law of partial pressures,the total pressure is the sum of the partial pressure of the dry gas and the vapor pressure of water: $P_{	ext{total}} = P_{O_2} + P_{H_2O}$.Given: $P_{	ext{total}} = 751\,mm\,Hg$ and $P_{H_2O} = 21\,mm\,Hg$.Therefore,$P_{O_2} = P_{	ext{total}} - P_{H_2O} = 751\,mm\,Hg - 21\,mm\,Hg = 730\,mm\,Hg$.To convert to $atm$: $P_{O_2} = \frac{730\,mm\,Hg}{760\,mm\,Hg/atm} \approx 0.96\,atm$.

$A$ sample of $O_2$ gas is collected over water at $23\,^oC$ and a barometric pressure of $751\,mm\,Hg$. What is the partial pressure of the $O_2$ gas in this sample? (Vapor pressure of water at $23\,^oC$ is $21\,mm\,Hg$)

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