Multiple choice

A methane + $H_2$ mixture contains 10 g methane and 5 g Hydrogen. If the pressure of the mixture is 30 atm. What is the partial pressure of $H_2$ in mixture.

  1. 6 atm

  2. 129 atm

  3. 24 atm

  4. 189 atm
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C Correct answer
Explanation

Moles of CH4 = 10/16 = 0.625. Moles of H2 = 5/2 = 2.5. Total moles = 3.125. Mole fraction of H2 = 2.5 / 3.125 = 0.8. Partial pressure of H2 = 0.8 * 30 atm = 24 atm.

AI explanation

The moles of methane are 10 g divided by 16 g/mol, equaling 0.625 moles, and the moles of hydrogen are 5 g divided by 2 g/mol, equaling 2.5 moles. This makes the total moles in the mixture 3.125, so the mole fraction of hydrogen is 2.5 divided by 3.125, which equals 0.8. Using Dalton's law, the partial pressure of hydrogen is 0.8 multiplied by the total pressure of 30 atm, resulting in 24 atm.

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