Answer:
Partial pressure of [tex]H_{2}[/tex] is 98 torr
Explanation:
Mole fraction (x) of a gas in mixture = (no. of moles of the gas)/(total no. of moles of gases in mixture)
Here, total no. of moles of gases in mixture = (0.02 + 0.02 + 0.1) moles = 0.14 moles
So, mole fraction of [tex]H_{2}[/tex] gas in mixture, [tex]x_{H_{2}}=[/tex] [tex]\frac{0.02}{0.14}=0.14[/tex]
Let's assume all three gases and their mixture behaves ideally.
Therefore, in accordance with Dalton's law of partial pressure for ideal gases-
[tex]P_{H_{2}}=x_{H_{2}}\times P_{total}[/tex]
Here, [tex]P_{H_{2}}[/tex] and [tex]P_{total}[/tex] are partial pressure of [tex]H_{2}[/tex] and total pressure of mixture respectively.
So, [tex]P_{H_{2}}=(0.14)\times (700torr)=98torr[/tex]
