In a flask containing 2 g of H_2 and 32 g o | vedclass

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(C) Step $1$: Calculate the number of moles of each gas.$n(H_2) = \frac{	ext{mass}}{	ext{molar mass}} = \frac{2 \ g}{2 \ g/mol} = 1 \ mol$.$n(SO_2)

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$2/3$ of total pressure

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(C) Step $1$: Calculate the number of moles of each gas.$n(H_2) = \frac{	ext{mass}}{	ext{molar mass}} = \frac{2 \ g}{2 \ g/mol} = 1 \ mol$.$n(SO_2) = \frac{32 \ g}{64 \ g/mol} = 0.5 \ mol$.Step $2$: Calculate the mole fraction of $H_2$.$x(H_2) = \frac{n(H_2)}{n(H_2) + n(SO_2)} = \frac{1}{1 + 0.5} = \frac{1}{1.5} = \frac{1}{3/2} = 2/3$.Step $3$: Use Dalton's Law of partial pressure.$P(H_2) = x(H_2) 	imes P_{	ext{total}} = \frac{2}{3} P_{	ext{total}}$.

In a flask containing $2 \ g$ of $H_2$ and $32 \ g$ of $SO_2$,the partial pressure of hydrogen is.....

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