22g of N2, 44 g of CO2 and 18 g of CH4 were put into a container of 750mm, calculate the partial pressure of each gas
To calculate the partial pressure of each gas, we first need to determine the number of moles of each gas using their respective molar masses. The molar masses of N2, CO2, and CH4 are 28g/mol, 44g/mol, and 16g/mol, respectively.
Moles of N2 = Mass of N2 / Molar mass of N2
= 22g / 28g/mol
= 0.79 mol
Moles of CO2 = Mass of CO2 / Molar mass of CO2
= 44g / 44g/mol
= 1 mol
Moles of CH4 = Mass of CH4 / Molar mass of CH4
= 18g / 16g/mol
= 1.13 mol
Next, we need to calculate the total number of moles of gas present in the container:
Total moles of gas = Moles of N2 + Moles of CO2 + Moles of CH4
= 0.79 mol + 1 mol + 1.13 mol
= 2.92 mol
Now, we can find the partial pressure of each gas using the ideal gas law, which states that the partial pressure of a gas is equal to the total pressure multiplied by the mole fraction of that gas.
Partial pressure of N2 = (Moles of N2 / Total moles of gas) * Total pressure
= (0.79 mol / 2.92 mol) * 750 mm
= 203.97 mm
Partial pressure of CO2 = (Moles of CO2 / Total moles of gas) * Total pressure
= (1 mol / 2.92 mol) * 750 mm
= 256.85 mm
Partial pressure of CH4 = (Moles of CH4 / Total moles of gas) * Total pressure
= (1.13 mol / 2.92 mol) * 750 mm
= 289.18 mm
Therefore, the partial pressure of N2 is 203.97 mm, the partial pressure of CO2 is 256.85 mm, and the partial pressure of CH4 is 289.18 mm.