Chapter 15 - Gases Flashcards
Absolute Zero
The lowest temperature that is theoretically possible, where the volume of gas equals 0 and there is no motion between particles (in theory).
Ideal Gas
A fictitious gas with no intermolecular forces, whose particles occupy negligible space.
Ideal Gas Equation
pV = nRT
where p = pressure in kPA
V = volume in L
n = amount in mol
R = universal gas constant (8.31)
T = temperature in kelvins
Kinetic Energy
The energy that an object possesses due to its motion.
Kelvin
A temperature scale increasing in the same increments as celsius, but starting at absolute zero. I.e. 0 K = -273 °C
Kinetic Molecular Theory
A model for the behaviour of gases which:
- composed of small particles that move rapidly in straight lines
- collisions between particles are elastic (no loss of kinetic energy)
- negligible intermolecular forces
- mostly empty space
- average kinetic energy increases as temp increases
Partial Pressure
The individual pressure of a specific gas in a mixture.
Pascal (Pa)
A unit of pressure, defined as 1 newton per metre squared.
Pressure (P)
The magnitude of force per unit of area. F/A
Maxell-Boltzmann Distribution
A graph representing the proportion of particles in a gas at a particular kinetic energy EK (bell curve shaped).
Diffusion
The spreading of gas particles to fill a volume of space evenly (rate dependent on temperature).
Dalton’s Law of Partial Pressures
The total pressure of a gas mixture is equal to the sum of the individual pressures of the gases in the mixture.
Pressure will increase if…
- amount of gas (in mol) is increased
- temperature is increased
- volume of container is decreased
Barometer
An instrument used to measure pressure.
Boyle’s Law
The volume of gas is inversely proportional to its pressure.
P1V1 = P2V2
