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(D) The partial pressure $(P_i)$ of a gas in a mixture is directly proportional to its number of moles $(n_i)$ according to Dalton's Law of Partial Pr

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$Ne$

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(D) The partial pressure $(P_i)$ of a gas in a mixture is directly proportional to its number of moles $(n_i)$ according to Dalton's Law of Partial Pressures ($P_i = x_i P_{total}$,where $x_i = \frac{n_i}{n_{total}}$). Number of moles $(n)$ is calculated as $n = \frac{	ext{mass}}{	ext{molar mass}}$. For $H_2$: $n = \frac{5 	ext{ g}}{2 	ext{ g/mol}} = 2.5 	ext{ mol}$. For $He$: $n = \frac{8 	ext{ g}}{4 	ext{ g/mol}} = 2.0 	ext{ mol}$. For $CO_2$: $n = \frac{50 	ext{ g}}{44 	ext{ g/mol}} \approx 1.136 	ext{ mol}$. For $Ne$: $n = \frac{20 	ext{ g}}{20 	ext{ g/mol}} = 1.0 	ext{ mol}$. Since $Ne$ has the minimum number of moles $(1.0 	ext{ mol})$,it exerts the minimum partial pressure.

$A$ container consists of a mixture of four gases: $5 \text{ g } H_2$,$8 \text{ g } He$,$50 \text{ g } CO_2$,and $20 \text{ g } Ne$ at a certain temperature. Which of the following gases exerts the minimum partial pressure?

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