A mixture of gases contains 0.235 mol CO2, 0.124 mol CO, and 0.326 mol O2. If the total
pressure of the mixture is 4.62 atm, what is the partial pressure of each gas?
XCO2 = mols CO2/total mols.
XCO = mols CO/total mols
XO2 = mols O2/total mols.
pCO2 = XCO2*Ptotal
pCO = XCO*Ptotal
pO2 = XO2*Ptotal
co2=1.58
co-0.836
o2-2.24
To find the partial pressure of each gas in the mixture, we need to use the concept of the mole fraction.
Mole fraction is defined as the ratio of the number of moles of a particular gas to the total number of moles of all the gases in the mixture.
First, we need to calculate the total number of moles of all the gases in the mixture:
Total moles of gases = 0.235 mol CO2 + 0.124 mol CO + 0.326 mol O2 = 0.685 mol
Next, we can calculate the mole fraction of each gas:
Mole fraction of CO2 = (0.235 mol CO2) / (0.685 mol) = 0.343
Mole fraction of CO = (0.124 mol CO) / (0.685 mol) = 0.181
Mole fraction of O2 = (0.326 mol O2) / (0.685 mol) = 0.476
Now that we have the mole fractions, we can calculate the partial pressures using the equation:
Partial pressure of a gas = Mole fraction of the gas * Total pressure
Partial pressure of CO2 = 0.343 * 4.62 atm = 1.582 atm
Partial pressure of CO = 0.181 * 4.62 atm = 0.836 atm
Partial pressure of O2 = 0.476 * 4.62 atm = 2.199 atm
Therefore, the partial pressure of CO2 is 1.582 atm, the partial pressure of CO is 0.836 atm, and the partial pressure of O2 is 2.199 atm.