Question

A mixture of 0.158 moles CO, 0.412 moles H2 and 0.710 moles O2 has a total pressure of 6.27 atm. What is the partial pressure of H2 (in atm)?

Answer 1

Answer:

≈ 2.02 atm

Explanation:

We can use the mole fraction of H2 to calculate its partial pressure in the mixture. The mole fraction of H2 is the number of moles of H2 divided by the total number of moles in the mixture:

moles of H2 = 0.412
total moles in mixture = 0.158 + 0.412 + 0.710 = 1.28

mole fraction of H2 = moles of H2 / total moles in mixture = 0.412 / 1.28 ≈ 0.322

The partial pressure of H2 can then be calculated using the total pressure of the mixture and the mole fraction of H2:

partial pressure of H2 = mole fraction of H2 x total pressure of mixture
partial pressure of H2 = 0.322 x 6.27 atm ≈ 2.02 atm

Therefore, the partial pressure of H2 in the mixture is approximately 2.02 atm.