In a mixture of $N_{2}$ and $C O_{2}$ gases, the partial pressure of $C O_{2}$ is 1.25 atm. The total pressure of the mixture is 5 atm.Find the mole fraction of $N_{2}$ in the mixture.

Q. A sealed vessel contains 0.5 moles of oxygen, 0.1 moles of carbon dioxide, and 0.4 moles of nitrogen gas. The total pressure of the gas mixture is 5 atm. What is the partial pressure of the carbon dioxide?

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A mixture of 2 moles of H2, 3 moles of NH3, 4 moles of CO2 and 5 moles of N2 exerts a total pressure of 798 torr. What is the partial pressure of CO2 gas ?

The correct option is C 228 torrTotal number of moles of the gases =2+3+4+5=14 mol Using Dalton's law of partial pressure p=Ptotal×χ Where, p=Partial pressure ptotal=Total vapour pressure Mole fraction of CO2=moles of CO2moles of solution=414 So, partial pressure of CO2 =798×414=228 torr

A mixture of $2$ moles of $H_{2}$ , $3$ moles of $N H_{3}$ , $4$ moles of $C O_{2}$ and $5$ moles of $N_{2}$ exerts a total pressure of $798$ torr. What is the partial pressure of $C O_{2}$ gas ?