A mixture of 0.5 text{ mol} N_2 gas, 1.0 text | vedclass

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(B) Step $1$: Calculate the total number of moles in the mixture.$n_{	ext{total}} = n_{N_2} + n_{O_2} + n_{H_2} = 0.5 + 1.0 + 1.5 = 3.0 	ext{ mol}$.

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$6$

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(B) Step $1$: Calculate the total number of moles in the mixture.$n_{	ext{total}} = n_{N_2} + n_{O_2} + n_{H_2} = 0.5 + 1.0 + 1.5 = 3.0 	ext{ mol}$.Step $2$: Calculate the mole fraction of $O_2$ $(x_{O_2})$.$x_{O_2} = \frac{n_{O_2}}{n_{	ext{total}}} = \frac{1.0}{3.0} = \frac{1}{3}$.Step $3$: Calculate the partial pressure of $O_2$ using Dalton's Law.$P_{O_2} = x_{O_2} 	imes P_{	ext{total}} = \frac{1}{3} 	imes 18 	ext{ bar} = 6.0 	ext{ bar}$.

$A$ mixture of $0.5 \text{ mol}$ $N_2$ gas, $1.0 \text{ mol}$ $O_2$ gas and $1.5 \text{ mol}$ $H_2$ gas exerts a total pressure of $18 \text{ bar}$. Find the partial pressure of $O_2(g)$. (in $\text{ bar}$)

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