A mixture of CO and N_2 gases of equal mass i | vedclass

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(A) The molar mass of both $CO$ and $N_2$ is $28 \, g/mol$.Since the masses are equal,the number of moles $(n = \frac{mass}{molar \, mass})$ for both

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$P_{N_2} = P_{CO}$

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(A) The molar mass of both $CO$ and $N_2$ is $28 \, g/mol$.Since the masses are equal,the number of moles $(n = \frac{mass}{molar \, mass})$ for both gases will be equal.According to Dalton's Law of Partial Pressures,the partial pressure of a gas is directly proportional to its mole fraction $(P_i = x_i 	imes P_{total})$.Since the number of moles of both gases is equal,their mole fractions are equal $(x_{CO} = x_{N_2} = 0.5)$.Therefore,the partial pressures are equal: $P_{CO} = P_{N_2}$.

$A$ mixture of $CO$ and $N_2$ gases of equal mass is filled in a cylinder. What will be the ratio of their partial pressures?

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