a mixture of gases contains 0.4 mole of N2, 0.5 moles of O2, and 0.7 moles of H2. What is the partial pressure of O2 if the total pressure is 1.3 atm?
There are several ways to do this. Probably the easiest is to use mole fractions.
total moles = 0.4 + 0.5 + 0.7 = 1.6 moles
mole fraction O2 = moles O2/total moles.
PO2 = XO2*Ptotal
To find the partial pressure of O2, we need to calculate the mole fraction of O2 in the mixture.
The mole fraction of a component is the ratio of the moles of that component to the total moles of all components.
First, we need to calculate the total moles of all components:
Total moles = moles of N2 + moles of O2 + moles of H2
= 0.4 + 0.5 + 0.7
= 1.6 moles
Next, we can calculate the mole fraction of O2:
Mole fraction of O2 = moles of O2 / Total moles
= 0.5 / 1.6
≈ 0.3125
Now, we can find the partial pressure of O2 using Dalton's law of partial pressures:
Partial pressure of O2 = Mole fraction of O2 x Total pressure
= 0.3125 x 1.3 atm
≈ 0.40625 atm
Therefore, the partial pressure of O2 in the mixture is approximately 0.40625 atm.
To find the partial pressure of O2, we need to use the mole fraction of O2 and the total pressure. The mole fraction of a gas is the ratio of moles of that gas to the total moles of all gases present in the mixture.
First, we need to calculate the total moles of gases present in the mixture:
Total moles = moles of N2 + moles of O2 + moles of H2
Total moles = 0.4 + 0.5 + 0.7
Total moles = 1.6 moles
Next, we determine the mole fraction of O2:
Mole fraction of O2 = moles of O2 / Total moles
Mole fraction of O2 = 0.5 / 1.6
Mole fraction of O2 ≈ 0.3125
Now, we can find the partial pressure of O2 using the mole fraction and the total pressure:
Partial pressure of O2 = Mole fraction of O2 × Total pressure
Partial pressure of O2 = 0.3125 × 1.3 atm
Partial pressure of O2 ≈ 0.40625 atm
Therefore, the partial pressure of O2 in the mixture is approximately 0.40625 atm.