CH15 Ideal gases

First assumption

- Made up of lots of particles moving in random directions at different speeds ( overall velocity is 0 m/s).

Second assumption

Time of collisions between particle is negligible compared to collisions between them.

Third assumption

Electrostatic forces are negligible except during collisions

Forth assumption

Collisions are perfectly elastic, momentum and kinetic energy are conserved.

Fifth assumption

The atoms of gas occupy negligible volume compared to the volume of gas.

Internal energy of a gas

The sum of kinetic and potential energies in an ideal gas (only internal energy is kinetic energy)

Temperature and kinetic energy relationship

Temperature and kinetic energy are directly proportional to each other (only if temperature is measured in kelvin).

Avogadro's constant (number)

6.022*10^23

Avogadro's constant definition

The amount of substance that contains the same amount of elementary entities as 0.012kg of carbon-12.

Boyle’s law equation

P1V1=P2V2 and PV=constant

Boyle’s law definition

Pressure of a fixed mass is inversely proportional to the volume if temperature remains constant.

Molar mass

the mass of one mole of a substance

Pressure and absolute temperature

they are directly proportional to each other

Combined gas law

PV/T = Constant P1V!/T1 = P2V2/T2

Ideal gas equation

PV = nRT (P = pressure (Pa), V = volume (m^3), n = moles (mol), R = molar gas constant (8.31 JK^-1), T = temperature (K))

root mean square speed

the square root of the average of the squared speeds of the gas molecules in a gas sample

root mean square speed formula

Vrms = 3RT/M rooted

Kinetic Theory of Gases equation

PV = 1/3nmc^2

Boltzmann constant

molar gas/ Avogadro's constant

2nd ideal gas equation

PV=nkNaT