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 of a gas collected over water is the sum of the partial pressure of the dry gas

Vedclass · Accepted Answer

$0.96\, atm$

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(C) According to Dalton's Law of Partial Pressures,the total pressure of a gas collected over water is the sum of the partial pressure of the dry gas and the vapour pressure of water at that temperature.$P_{	ext{total}} = P_{O_2} + P_{H_2O}$Given:$P_{	ext{total}} = 751\, mm\, Hg$$P_{H_2O} = 21\, mm\, Hg$Therefore,$P_{O_2} = P_{	ext{total}} - P_{H_2O} = 751 - 21 = 730\, mm\, Hg$.To convert this to atmospheres,we use the relation $1\, atm = 760\, mm\, Hg$:$P_{O_2} = \frac{730}{760}\, atm \approx 0.96\, atm$.

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

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