What ratio by mass of Ne and CH_4 should be m | vedclass

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(B) The partial pressure of a gas is given by $P_i = x_i P_{total}$, where $x_i$ is the mole fraction.For the partial pressures to be equal $(P_{Ne} =

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$5:4$

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(B) The partial pressure of a gas is given by $P_i = x_i P_{total}$, where $x_i$ is the mole fraction.For the partial pressures to be equal $(P_{Ne} = P_{CH_4})$, their mole fractions must be equal $(x_{Ne} = x_{CH_4})$.Since $x_i = \frac{n_i}{n_{total}}$, equal mole fractions imply equal number of moles $(n_{Ne} = n_{CH_4})$.Let the number of moles be $n$. The mass of $Ne$ is $m_{Ne} = n 	imes M_{Ne} = n 	imes 20 \ 	ext{g/mol}$.The mass of $CH_4$ is $m_{CH_4} = n 	imes M_{CH_4} = n 	imes 16 \ 	ext{g/mol}$.The ratio by mass is $\frac{m_{Ne}}{m_{CH_4}} = \frac{20n}{16n} = \frac{5}{4}$ or $5:4$.

What ratio by mass of $Ne$ and $CH_4$ should be mixed so that the partial pressure exerted by each gas is the same?

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