A gaseous mixture contains 65% N_2,15% O_2,an | vedclass

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(C) According to Dalton's Law of Partial Pressures,the partial pressure of a gas is equal to its mole fraction multiplied by the total pressure. Since

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$494, 114, 152$

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(C) According to Dalton's Law of Partial Pressures,the partial pressure of a gas is equal to its mole fraction multiplied by the total pressure. Since the mixture is given by volume percentage,the mole fraction is equal to the volume fraction.$P_{N_2} = 760 	imes \frac{65}{100} = 494 \, mm \, Hg$$P_{O_2} = 760 	imes \frac{15}{100} = 114 \, mm \, Hg$$P_{CO_2} = 760 	imes \frac{20}{100} = 152 \, mm \, Hg$

$A$ gaseous mixture contains $65\%$ $N_2$,$15\%$ $O_2$,and $20\%$ $CO_2$ by volume at a total pressure of $760 \, mm \, Hg$. Calculate the partial pressure of each gas in $mm \, Hg$.

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