What will be the pressure of the gaseous mixt | vedclass

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(B) According to Boyle's Law,$p_{1}V_{1} = p_{2}V_{2}$ at constant temperature.For $H_{2}$:$p_{1} = 0.8 \, bar, V_{1} = 0.5 \, L, V_{2} = 1 \, L$$p_{H

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$1.8$

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(B) According to Boyle's Law,$p_{1}V_{1} = p_{2}V_{2}$ at constant temperature.For $H_{2}$:$p_{1} = 0.8 \, bar, V_{1} = 0.5 \, L, V_{2} = 1 \, L$$p_{H_{2}} = \frac{0.8 	imes 0.5}{1} = 0.4 \, bar$For $O_{2}$:$p_{1} = 0.7 \, bar, V_{1} = 2.0 \, L, V_{2} = 1 \, L$$p_{O_{2}} = \frac{0.7 	imes 2.0}{1} = 1.4 \, bar$According to Dalton's Law of Partial Pressures,the total pressure $p_{total} = p_{H_{2}} + p_{O_{2}}$.$p_{total} = 0.4 \, bar + 1.4 \, bar = 1.8 \, bar$.

What will be the pressure of the gaseous mixture when $0.5 \, L$ of $H_{2}$ at $0.8 \, bar$ and $2.0 \, L$ of dioxygen at $0.7 \, bar$ are introduced in a $1 \, L$ vessel at $27^{\circ} C$ (in $, bar$)?

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