Chapter 10- Gases Flashcards
(23 cards)
A process by which gas particles pass through a tiny opening
Effusion
Spontaneous Mixing of the particles of two substances caused by the random motion
Diffusion
A collision between gas particle and between gas particles and container walls in which there is no net loss of kinetic energy
elastic collision
A substance that can flow and therefore take the shape of its container; a liquid or a gas
Fluids
An imaginary gas that perfectly fits all the assumptions of the kinetic molecular theory
Ideal gas
A theory based on the idea that particles of matter are always in motion
Kinetic molecular theory
A gas that does not behave completely according to the assumptions of the kinetic molecular theory
Real gas
Exactly equivalent to 760 mmHg
Atmosphere of pressure
A device used to measure atmospheric pressure
Barometer
A common unit of measure
mmHg
The SI unit for force
Newton
The pressure exerted by a force of one newton
acting on an area of 1 m²
Pascal
The force per unit area on a surface
Pressure
The agreed-upon standard conditions of exactly 1 atm of pressure and 0°C
Standard temperature and pressure
A pressure of 1 mmHg
Torr
The temperature -273.15°C, Given a value of zero in the Kelvin scale
Absolute zero
The volume of a fixed mass of gas varies inversely with pressure at constant temperature
Boyles law
The volume of a fixed mass of gas at constant pressure varies directly with the Kelvin temperature
Charles law
The relationship between the pressure, volume, and temperature of a fixed amount of gas
Combined gas law
The total pressure of a mixture of gases is equal to the sum of the partial pressures of the component gases
Dalton’s law of partial pressures
Simple mathematical relationships between the volume, temperature, pressure, and quantity of a gas
Gas laws
The pressure of a fixed mass of gas at constant volume varies directly with the Kelvin temperature
Gay Loussac’s law
The pressure of each gas in a mixture
Partial pressure
