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Chemistry Unit 5

Unit 5: Gas Laws + Stoichiometry 2

TermDefinition
Kinetic Energy Energy in motion
Temperature A measure of the average kinetic energy of a substance
Absolute Zero The temperature at which particles have zero kinetic energy
Thermal Energy The sum kinetic energy of a sample of matter (more partial motion if there is more energy added)
Heat An energy transfer due to a temperature difference (heat always transfers from high to low temperature)
Pressure Force per unit area
Gas Pressure Depends on the number of collisions between gas molecules and the walls of their container
Atmosphere atm
Boyle's Gas Law Volume and pressure are inversely proportional at constant temperature (P1V1=P2V2)
Charles' Gas Law Volume and absolute temperature are directly proportional at constant pressure (V1/T1=V2/T2, must be measured in Kelvin)
The Ideal Gas Law PV=nRT
Avogadro's Law The volume of any gas is directly proportional to the number of moles of the gas (at constant temp. and pressure) (V1/n1=V2/n2)
P Pressure (atm) of gas
V Volume of container (liters)
n Moles (mol) of gas
R Universal gas law constant (0.0821 L x atm/mol x K)
T Temperature (Kelvin) of gas
Standard Temperature and Pressure (STP) P = 1 atm, T = 273.15
Moles Mass/molar mass, m/Mr=n, Mr=mRT/PV
Density mass/volume, d=m/v, d=Mr x P/RT
Kinetic Molecular Theory (KMT) Gases consist of tiny particles in constant, random motion
SI Unit Pa (Pascal) - measured with barometer
Directly Proportional both quantities increase together
Inversely Proportional one quantity increases, while the other decreases
Fahrenheit T°F = T°C x (9/5) + 32
Kelvin TK = T°C + 273.15
Created by: sara!
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