According to Dalton’s Law, the total pressure inside a container is obtained by adding all the partial pressures of each non-reacting gas.
Concept #1: Understanding Dalton's Law
Concept #2: Understanding mole fraction and partial pressure
The partial pressure of a gas is based on the moles of that gas. The relationship of the different moles of gases helps us determine the mole fraction of each gas.
Example #1: A container has 16.7 g O2, 8.1 g H2 and 35.2 g N2 and contains a total pressure of 0.83 atm. Calculate the mole fraction of O2 and its partial pressure.
Practice: A gas mixture with a total pressure of 812 mmHg contains the following gases at with their partial pressures: Cl2 = 210 mmHg, H2 = 180 mmHg, CO2 = 215 mmHg. If argon gas is also present calculate its mole fraction.