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, you know the total pressure of a gas mixture, you can use the number of moles to find the partial or the partial pressures to find the number of moles. Example Problem: A mixture of N_2, O_2, and He gases Part A A mixture of He. Ar, and Xe has a total pressure of 2.60 atm. The partial pressure of He is 0.300 atm, and the partial pressure of Ar is 0.350 atm. What is the partial pressure of Xe? Part B A volume of 18.0 L contains a mixture of 0.250 mole N_2, 0250 mole O_2, and an unknown quantity of He. The temperature of the mixture is 0 degree C, and the total pressure is 1.00 atm. How many grams of helium are present in the gas mixture?

Explanation / Answer

B)

First, identify total mols via ideal gas law

PV = nRT

n = PV/(RT)

T = 0°C = 273 K

n = (1*18)/(0.082*273) = 0.80407 mol

note that

Total mol = N2 + O2 + He = 0.80407

0.80407 = 0.25 + 0.25 + He

He moles = 0.80407 - 0.5 = 0.30407 mol of He

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