A mixture of krypton and methane gases, at a total pressure of 775 mm Hg, contains 4.77 grams of krypton and 2.38 grams of methane. What is the partial pressure of each gas in the mixture?

Partial pressure of Kr → 214.06 mmHg

Partial pressure of CH₄ → 560.5 mmHg

Explanation:

To determine partial pressure we can work with mole fraction.

Mole fraction = moles of gas / Total gas = Partial pressure gas / Total pressure

Let's determine the moles of each compound (mass / molar mass)

4.77 g / 83.80 g/mol = 0.0569 moles of Kr

2.38 g / 16 g/mol = 0.149 moles of CH₄

Total moles = 0.0569 + 0.149 → 0.206

Partial pressure of Kr → (0.0569/0.206). 775 mm Hg = 214.06 mmHg

Partial pressure of CH₄ → (0.149/0.206). 775 mm Hg = 560.5 mmHg