Multiple Choice
A gas mixture contains each of the following gases at the indicated partial pressures: N₂, 257 Torr; O₂, 189 Torr; and He, 107 Torr. What is the total pressure of the mixture?
7. Gases
Partial Pressure
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A mixture of 7.87 g CH4 and 7.13 g Xe is placed in a container, and the total pressure is found to be 0.51 atm. Determine the partial pressure of Xe in atm.
A
0.36 atm
B
0.24 atm
C
0.48 atm
D
0.12 atm
Verified step by step guidance1
Calculate the number of moles of CH4 using its molar mass. The molar mass of CH4 is approximately 16.04 g/mol. Use the formula: \( \text{moles of CH4} = \frac{7.87 \text{ g}}{16.04 \text{ g/mol}} \).
Calculate the number of moles of Xe using its molar mass. The molar mass of Xe is approximately 131.29 g/mol. Use the formula: \( \text{moles of Xe} = \frac{7.13 \text{ g}}{131.29 \text{ g/mol}} \).
Determine the total number of moles in the mixture by adding the moles of CH4 and Xe together.
Use Dalton's Law of Partial Pressures to find the partial pressure of Xe. According to Dalton's Law, the partial pressure of a gas is equal to the mole fraction of the gas multiplied by the total pressure. Calculate the mole fraction of Xe: \( \text{mole fraction of Xe} = \frac{\text{moles of Xe}}{\text{total moles}} \).
Calculate the partial pressure of Xe using the formula: \( \text{partial pressure of Xe} = \text{mole fraction of Xe} \times 0.51 \text{ atm} \).
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