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(C) According to Dalton's Law of Partial Pressures,the total pressure $P_{Total}$ is the sum of partial pressures of individual gases: $P_{Total} = P_

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$0.45$ and $0.55$

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(C) According to Dalton's Law of Partial Pressures,the total pressure $P_{Total}$ is the sum of partial pressures of individual gases: $P_{Total} = P_A + P_B = 4.5 \ bar + 5.5 \ bar = 10.0 \ bar$. The mole fraction $x_i$ of a gas is given by the ratio of its partial pressure to the total pressure: $x_A = \frac{P_A}{P_{Total}} = \frac{4.5 \ bar}{10.0 \ bar} = 0.45$. Similarly,for gas $B$: $x_B = \frac{P_B}{P_{Total}} = \frac{5.5 \ bar}{10.0 \ bar} = 0.55$. Therefore,the mole fractions of $A$ and $B$ are $0.45$ and $0.55$ respectively.

$A$ closed container contains a mixture of non-reacting gases $A$ and $B$. The partial pressures of $A$ and $B$ are $4.5 \ bar$ and $5.5 \ bar$ respectively. Find the mole fractions of $A$ and $B$ respectively.

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