chapter 10 chemistry

pressure

the amount of force exerted per unit area of a surface

newton

SI unit of force

barometer

An instrument that measures atmospheric pressure

millimeters of mercury

unit of pressure

atmosphere of pressure

exactly equivalent to 760 mm Hg; weight of the atmosphere; unit of pressure

pascal

SI unit of pressure

standard temperature and pressure

for a gas, the temperature of 0 Celsius and pressure 1.00 atmosphere

torr

unit of pressure; 760 = 1 atm

Kinetic Molecular Theory

based on the idea that particles of matter are always in motion

ideal gas

an imaginary gas that perfectly fits all the assumptions of the kinetic-molecular theory

elastic collision

collisions between gas particles and container walls; no net loss of kinetic energy

fluids

liquids and gases that flow

diffusion

spontaneous mixing of the particles of two substances caused by their random motion

effusion

A process by which gas particles pass through a tiny opening

real gas

a gas that does not behave completely according to the assumptions of the kinetic-molecular theory

gas laws

simple mathematical relationships between the volume, temperature, pressure, and amount of a gas

boyle’s law

states that the volume of a fixed mass of gas varies inversely with the pressure at constant temperature

absolute zero

temperature -273.15 degrees C is given a value of zero on the Kelvin scale

Charles’s law

states that the volume of a fixed mass of gas at constant pressure varies directly with the kelvin temperature

gay-lussac’s law

the pressure of a fixed mass of gas at constant volume varies directly with the kelvin temperature

combined gas law

expresses the relationship between pressure, volume, and temperature of a fixed amount of gas

partial pressure

pressure of each gas in a mixture

dalton’s law of partial pressures

states that the total pressure of a mixture of gases is equal to the sum of the partial pressure of the component gases