A mixture of krypton and oxygen gases, at a total pressure of 942 mm Hg, contains 17.7 grams of krypton and 4.13 grams of oxygen. What is the partial pressure of each gas in the mixture?
To find the partial pressures of each gas in the mixture, we need to first calculate the moles of each gas present using the given masses and molar masses.
1. Calculate the molar masses of krypton (Kr) and oxygen (O2):
- Molar mass of Kr = 83.80 g/mol
- Molar mass of O2 = 32.00 g/mol
2. Calculate the moles of each gas present in the mixture:
- Moles of Kr = 17.7 g / 83.80 g/mol = 0.211 mol
- Moles of O2 = 4.13 g / 32.00 g/mol = 0.129 mol
3. Calculate the mole fraction of each gas:
- Mole fraction of Kr = 0.211 mol / (0.211 mol + 0.129 mol) = 0.621
- Mole fraction of O2 = 0.129 mol / (0.211 mol + 0.129 mol) = 0.379
4. Calculate the partial pressures of each gas using their mole fractions and the total pressure of the mixture:
- Partial pressure of Kr = 0.621 x 942 mm Hg = 585.402 mm Hg
- Partial pressure of O2 = 0.379 x 942 mm Hg = 356.598 mm Hg
Therefore, the partial pressure of krypton is 585.402 mm Hg and the partial pressure of oxygen is 356.598 mm Hg in the mixture.