In what ratio by mass carbon dioxide (CO_2) a | vedclass

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(B) According to Dalton's law of partial pressure,$P_i = x_i 	imes P_{total}$,where $x_i$ is the mole fraction of the gas.For the partial pressures t

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$11:7$

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(B) According to Dalton's law of partial pressure,$P_i = x_i 	imes P_{total}$,where $x_i$ is the mole fraction of the gas.For the partial pressures to be equal $(P_{CO_2} = P_{N_2})$,their mole fractions must be equal $(x_{CO_2} = x_{N_2})$.Since $x_i = \frac{n_i}{n_{total}}$,equal mole fractions imply that the number of moles must be equal $(n_{CO_2} = n_{N_2})$.Let the number of moles be $n$.Mass of $CO_2 = n 	imes 	ext{Molar mass of } CO_2 = n 	imes 44 \ g/mol$.Mass of $N_2 = n 	imes 	ext{Molar mass of } N_2 = n 	imes 28 \ g/mol$.The ratio of masses = $\frac{n 	imes 44}{n 	imes 28} = \frac{44}{28} = \frac{11}{7}$.

In what ratio by mass carbon dioxide $(CO_2)$ and nitrogen $(N_2)$ should be mixed so that the partial pressure exerted by each gas is the same?

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