Chapter 8 - Gases
Conversion factors for pressure
1 atm = 760 mmHg
760 torr = 760 mmHg
1 atm = 14.7 lb./in. (psi)
1 atm = 101.325 kPa
#1 Kinetic molecular theory of gas
A gas consists of small particles that move randomly with high velocities.
#2 Kinetic molecular theory of gas
The attractive forces between the particles of gas are usually very small.
#3 Kinetic molecular theory of gases
The actual volume occupied by gas molecules is extremely small compared with the volume that the gas occupies.
#4 Kinetic molecular theory of gases
Gas particles are in constant motion, moving rapidly in straight paths.
#5 Kinetic molecular theory of gases
The average kinetic energy of gas molecules is proportional to the Kelvin temperature.
P1V1 = P2V2
Pressure and Volume
If pressure increases, volume decreases and vice versa.
V1/T1 = V2/T2
Temperature and Volume
If temperature increases, then volume increases and vice versa.
P1/T1 = P2/T2
Temperature and Pressure
if temperature increases, then pressure increases, and vice versa.
The Combined Gas Law
P1V1/T1 = P2V2/T2
V1/n1 = V2/n2
Volume and Moles
PT = P1 + P2 + P3 + . . .
22.4 L = 1 mole of gas at STP