Chemistry Learning Targets – Chapter 11

explains gas behavior. gases made of tiny particles far apart relative to their size. particles are in continuous random motion.

no force of attraction or repulsion between particles. average kinetic energy of particles depends on temperature.

collisions between particles and container or other particles

hypothetical gas whose P, V, and T behavior is completely described by the ideal-gas equation.

low density, indefinite shape/volume, compressibility and expandability, diffusivity and pressure

the spread of one substance throughout a space throughout a second substance

the escape of gas molecules through a tiny hole into an evacuated space

a gas that does not behave as an ideal gas due to interactions between gas molecules

the force acting upon an object. different than force since this depends upon how much of an area the force is being exerted upon.

unit for force

f/a

measures pressure

1 atm, 273 K (0 C)

pressure, volume, temperature

relationship between P and V. inverse relationship. when p increases, v decreases. P1V1=P2V2

relationship between V and t. when v increases, t increases. direct relationship.

V1/T1=V2/T2

lowest temperature ever on the Kelvin scale. 0 K = 273 C

relationship between P and T. when p increases, t increases. direct relationship. P1/T1 = P2/T2

P1V1/T1 = P2V2/T2

the pressure exerted by a particular component of a gas mixture.

Ptotal = P1 + P2 + P3 + ....

at a given temperature and pressure, the volumes of gases that react with one another are ratios of small whole numbers.

the volume of a gas at a given temperature and pressure is directly proportional to the number of moles of gas.

V = constant x n

standard molar volume of a gas

PV = nRT

rate1 / rate2 = square root of MM2/MM1