Agenda Ideal Gas Law Gas Laws Review Gas Laws Practice
Gas Variables Four variables to describe a gas: Pressure (P) Volume (V) Temperature (T) Amount (n)
Ideal Gas Law Four variables to describe a gas: Pressure (P) Volume (V) Temperature (T) Amount (n)
Ideal Gas Law PV = nRT P = Pressure V = Volume n = Number of Moles R = Gas Constant (Always Provided!) T = Temperature
Ideal Gas Law Relationships PV = nRT As Pressure Increases, Temperature Increases By extension – As Pressure Decreases Temperature Decreases As Volume Increases, Temperature AND Pressure Decrease By extension – As Volume Decreases, Temperature and Pressure Increase As Amount (number of moles) Increases, Pressure and Temperature Increase By extension – As Amount Decreases, Pressure and Temperature Decrease
The initial temperature of a 1.0 L sample of argon is 20.° C. The pressure is decreased from 720 mm Hg to 360 mm Hg and the volume increases to 2.14 L. What was the change in temperature of the argon? PV = nRT R = L mmHg K −1 mol −1 mmHg
Kinetic Molecular Theory Postulates 1. Gases consist of tiny particles. 2. These particles are so small, compared with the distances between them, that the volume (size) of the individual particles can be assumed to be negligible (zero). 3. The particles are in constant random motion, colliding with the walls of the container. These collisions with the walls cause the pressure exerted by the gas. 4. The particles are assumed not to attract or to repel each other. 5. The average kinetic energy of the gas particles is directly proportional to the temperature of the gas.
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