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(A) Let the mass of both $CO$ and $N_2$ be $w \ g$.The molar mass of $CO$ is $28 \ g/mol$ and the molar mass of $N_2$ is $28 \ g/mol$.The number of mo

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$P_{CO} = P_{N_2}$

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(A) Let the mass of both $CO$ and $N_2$ be $w \ g$.The molar mass of $CO$ is $28 \ g/mol$ and the molar mass of $N_2$ is $28 \ g/mol$.The number of moles is given by $n = \frac{	ext{mass}}{	ext{molar mass}}$.$n_{CO} = \frac{w}{28}$ and $n_{N_2} = \frac{w}{28}$.According to Dalton's Law of partial pressure,$P_i = x_i 	imes P_{total}$,where $x_i$ is the mole fraction.Since $n_{CO} = n_{N_2}$,the mole fractions are equal $(x_{CO} = x_{N_2} = 0.5)$.Therefore,the partial pressures are equal: $P_{CO} = P_{N_2}$.

$A$ cylinder is filled with a gaseous mixture containing equal masses of $CO$ and $N_2$. What will be the ratio of their partial pressures?

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