To use partial pressure in gas law calculations. In a mixture of gases, the tota

Question

To use partial pressure in gas law calculations. In a mixture of gases, the total pressure of the gas mixture is equal to the sum of the partial pressures of the individual gases. For example, if you have a mixture of helium at 2 atm and argon at 4 atm, then the total pressure of the gas inside the cylinder is 6 atm. Similarly, if you know the total pressure of a gas mixture, you can use the number of moles to find the partial pressures, or the partial pressures to find the number of moles. Example Problem: A mixture of N_2, O_2, and He gases has a total pressure of 1 atm. The partial pressures of N_2 and O_2 are 0.7 atm and 0 25 atm, respectively. What is the portal pressure of He? The sum of the partial pressures is equal to the total pressure; P_total = P_N_2 = P_N_2+ P_O_2 + P_He Rearranging this equation, the partial pressure of He is P_He = P_total - P_N_2 - P_O_2 = 1.00 atm - 0.70 atm - 0.25 atm = 0.05 atm A mixture of He, Ar, and Xe has a total pressure of 3.00 atm. The partial pressure of He is 0.450 atm, and the partial pressure of Ar is 0.450 atm. What is the partial pressure of Xe? Express your answer to three significant figures and include the appropriate units.

Explanation / Answer

Total pressure = Sum of the partial pressures of all the gases

3 = 0.45 + 0.45 + pXe

pXe = 3-0.9 = 2.1 atm

So

pXe = 2.1 atm

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