The Gas Laws Flashcards
Kinetic Energy
Energy of motion
KE=1/2mv^2
Kinetic Molecular Theory (KMT)
Gases consist of tiny particles in constant, random motion
Temperature
A measure of the average kinetic energy of a substance
Absolute Zero
The temperature at which particles have zero kinetic energy
Fahrenheit Temperature Scale for water
Boiling: 212
Freezing: 32
Absolute Zero: -459.67
Celsius Temperature Scale for water
Boiling: 100
Freezing: 0
Absolute Zero: -273.15
Kelvin Temperature Scale for water
Boiling: 373.15
Freezing: 273.15
Absolute zero: 0
Thermal energy
The sum kinetic energy of a sample of matter
Particle motion increases with the addition of energy
Pressure
Force per unit area
⭐️Gas pressure
Depends on the number of collisions between gas molecules and the walls of the container
SI unit
Pa(pascal)
Boyle’s gas law
Volume and pressure are inversely proportional at constant temperature
P1V1=P2P2
Charles’ gas law
Volume and absolute temperature are directly proportional at constant pressure
V1/T1=V2/V2
T= temperature ( must be expressed in KELVIN)
Combined Gas Law
P1V1/T1=P2V2/T2
Standard Temperature and Pressure (STP)
- p= 1 atm or 101.324kPa or 760 torr or 760 mm Hg
- T= 273.15 K
The Ideal Gas Law
PV=nRT
Combines 3 laws into 1
1: Boyles Law
2: Charles’ Lae
3. Avogadros Law
-the volume of any gas is directly proportional to number of moles of that gas(at constant temp and pressure)
PV=nRT
P= pressure (atm) of gas
V= volume of container (liters)
n= moles (mol) of gas
R= universal gas law constant
T= temperature
Universal Gas Law Constant
0.0821 Latm/molK
