Question

A vessel of volume 100 cm3 contains 0.25 mol o2 and 0.034 mol co2 at 10.0c. Calculate the partial pressure of each component and their total pressure

Answer 1

Answer: The partial pressure of oxygen is 76.56 atm , partial pressure of carbon dioxide is 10.44 atm and the total pressure is 87 atm.

Step-by-step explanation:

According to the ideal gas equation:'

`PV=nRT`

P = Pressure of the gas = ?

V= Volume of the gas =
`100cm^3=0.1L`
`1L=1000cm^3`

T= Temperature of the gas = 10°C = 373 K

R= Gas constant = 0.0821 atmL/K mol

n= moles of gas= 0.25 +0.034 = 0.284 moles

`P=(nRT)/(V)=(0.284* 0.0821* 373)/(0.1)=87atm`

`x_(O_2)` = mole fraction of oxygen=
`\frac{\text {moles of }O_2}{\text {moles of }O_2+\text{moles of }CO_2}=(0.25)/(0.25+0.034)=0.88`,

`x_(CO_2)` =mole fraction of carbon dioxide=
`\frac{\text {moles of }CO_2}{\text {moles of }O_2+\text{moles of }CO_2}=(0.034)/(0.25+0.034)=0.12`

partial pressure of oxygen =
`p_(O_2)=x_(O_2)* P=0.88* 87=76.56atm`

partial pressure of carbon dioxide=
`p_(CO_2)=x_(CO_2)* P=0.12* 87=10.44atmatm`

The partial pressure of oxygen is 76.56 atm , partial pressure of carbon dioxide is 10.44 atm and the total pressure is 87 atm.