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Temperature
A measure of the average kinetic energy of particles
Standard Temperature
0C (273K)
Pressure
The force per unit area on a surface
Standard Pressure
1 atm (101.3 kPa) (760 mmHg) (760 torr)
Absolute Zero
The theoretical temperature where the motion of particles cease, would have no kinetic energy
STP
Standard Temperature and Pressure
Gas Laws
The simplest mathematical relationships between the volume, temperature, pressure and amount of a gas
Boyle’s Law
The volume of a fixed mass of gas varies inversely with the pressure at constant temperature (P1*V1 = P2*V2)
Charles’s Law
The volume of a fixed mass of gas at constant pressure varies directly with the kelvin temperature (V1/T1 = V2/T2)
Gay-Lussac’s Law
The pressure of a fixed mass of gas at constant volume varies directly with the kelvin temperature (P1/T1 = P2/T2)
The Combined Gas Law
Describes the relationship among the pressure, temperature, and volume of an enclosed gas ((P1*V1)/T1 = (P2*V2)/T2)
Avogadro’s Law
Equal volumes of gases at the same temperature ad pressure contain equal numbers of molecules (22.4L)
Molar Volume
1 mole of a gas at STP = 22.4 L
large numbers of tiny particles that are far apart
Gases consist of…
elastic collisions
Collisions between gas particles and between particles and container walls are…
no net loss
Elastic collisions have _______ of kinetic energy
continuous
Gas particles are in _____ motion
no forces
There are _ __ of attraction or repulsion between gas particles
average kinetic energy
The ____ of gas particles depends on the temperature of the gas
Note 
Flashcard (46)