 or or taken why

Make sure to remember your password. If you forget it there is no way for StudyStack to send you a reset link. You would need to create a new account.

Don't know
Know
remaining cards
Save
0:01
Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.

Normal Size     Small Size show me how

# Honors Chem Ch 10

Diffusion Spontaneous mixing of the particles of two substances caused by their random motion
Effusion A process by which gas particles under pressure pass through a tiny opening
Elastic Collision A collision between gas particles and between gas particles and container walls in which there is no net loss of kinetic energy
Fluid A substance that can flow and therefore take the shape of its container; a liquid or gas
Ideal Gas An imaginary gas that perfectly fits all the assumptions of the kinetic-molecular theory
Kinetic-Molecular Theory A theory based on the idea that particles of matter are always in motion
Real Gas A gas that does not behave completely according to the assumptions of the kinetic-molecular theory
Atmosphere of Pressure Exactly equivalent to 760 mmHg
Barometer A device used to measure atmospheric pressure
Millimeter of Mercury A common unit of pressure
Newton The SI unit for force; the force that will increase the speed of a one kilogram mass by one meter per second each second it is applied
Pascal The pressure exerted by a force of one newton acting on an area of one square meter
Pressure The force per unit area on a surface
Standard Temperature and Pressure The agreed-upon standard conditions of exactly 1 atm pressure and 0 degrees C
Absolute Zero The temperature -273.15 degrees C, given a value of zero in the Kelvin scale
Boyle's Law The volume of a fixed mass of gas varies inversely with pressure at constant temperature
Charles's Law The volume of a fixed mass of gas at constant pressure varies directly with the Kelvin temperature
Combined Gas Law The relationship between the pressure, volume, and temperature of a fixed amount of gas
Dalton's Law of Partial Pressures The total pressure of a mixture of gases is equal to the sum of the partial pressures of the component gases
Gas Laws Simple mathematical relationships between the volume, temperature, pressure, and quantity of a gas
Gay-Lussac's Law The pressure of a fixed mass of gas at constant volume varies directly with the Kelvin temperature
Partial Pressure the pressure of each gas in a mixture
Created by: kost