Partial Pressure Practice Problems PDF

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Really good practice for General Chemistry 1! ...

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Partial Pressure Practice Problems Formulas: PT = P1 + P2 + … P1 = X1PTotal X1 = (n1/nTotal) 1. A mixture of 2.00 moles of H2, 3.00 moles of NH3, 4.00 moles of CO2 and 5.00 moles of N2 exerts a total pressure of 800.0 torr. What is the partial pressure of each gas? 2. The partial pressure of F2 is 300.0 torr in a mixture of gases where the total pressure is 1.00 atm. What is the mole fraction of F2? 3. What’s the partial pressure of carbon dioxide in a container that holds 5 moles of carbon dioxide, 3 moles of nitrogen, and 1 mole of hydrogen and has a total pressure of 1.05 atm? 4. A container with two gases, helium and argon, is 30.0% by volume helium. Calculate the partial pressure of helium and argon if the total pressure inside the container is 4.00 atm. 5. If 3 moles of N2 and 4 moles of O2 are placed in a 35.0 L container at a temperature of 25 ℃, what will the pressure of the resulting mixture of gases be?

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1. Answers to Question #1 a. PH2 = 114 torr b. PNH3 = 171 torr c. PCO2 = 229 torr 2. 3. 4. 5.

d. PN2 = 286 torr 0.395 0.58 atm 1.20 atm He; 2.80 atm Ar 4.88 atm...