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# Dalton's Law: Partial Pressure (Simplified)

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Sections
Pressure Units
Kinetic Molecular Theory
The Ideal Gas Law
The Ideal Gas Law Derivations
The Ideal Gas Law Applications
Chemistry Gas Laws
Chemistry Gas Laws: Combined Gas Law
Standard Temperature and Pressure
Dalton's Law: Partial Pressure (Simplified)
Gas Stoichiometry
Intermolecular Forces (Simplified)
Intermolecular Forces and Physical Properties
Atomic, Ionic and Molecular Solids
Heating and Cooling Curves

Partial Pressure (PGas) is the pressure exerted by an individual gas within a container.

###### Partial Pressure of Gases

Concept #1: Partial Pressure

In a container of unreacting gases, total pressure of the container is the sum of the partial pressures of each gas. Example #1: A sample of neon gas exerts a pressure of 1.85 atm inside a cylinder. Some nitrogen gas is also present, at a pressure of 500 torr. What is the total pressure inside the cylinder?

Concept #2: Using moles to determine Partial Pressure

Example #2: If 12.0 g helium and 20.0 g oxygen are placed inside a 5.0 L cylinder at 30 ºC, what is the partial pressure of the helium gas?

Concept #3: Fractional Composition to Partial Pressure

Example #3: A cylinder of a gas mixture used for calibration of blood gas analyzers in medical laboratories contains 5.0% CO2, 12.0% O2, and the remainder N2 at a total pressure of 146 atm. What is the partial pressure of each component of this gas?

Practice: A gas mixture contains 72.8% chlorine and 27.2% neon by mass. What is the partial pressure of neon in the mixture if the total pressure is recorded as 809 mmHg?

Practice: The partial pressure of N2 in the air is 593 mmHg at 1 atm. What is the partial pressure of N2 in a bubble of air a scuba diver breathes when he is 66 ft below the surface of the water where the pressure is 3.00 atm?