Ideal gas molecules

Name the 4 points in the kinetic theory of gases

• particles in a gas are in a constant state of random motion.

• particles in a gas collide with each other, and the walls of a container, without transferring kinetic energy.

• temperature of the gas related to average kinetic energy of the particles.

• as kinetic energy of particles increase, temperature of gas increases.

explain gas pressure in a container

gas particles collide with the wall of the container, and exert a force.

explain the effect temperature increase of a gas, with pressure inside a container

gas particles have more kinetic energy…

1. they collide with the container with more force (increases energy of collisions)

2. increases the number of collisions

therefore, pressure increases

explain the change in pressure when you decrease the volume of a container

1. less distance for gas particles to travel.

2. collide with container more frequently.

   therefore, pressure increases

the coldest temperature you can ever get anything is -273 degrees Celsius, this is called…

Absolute zero

Absolute Zero = start of the Kelvin scale

degrees Celsius → Kelvins

+ 273

Kelvins → Degrees Celsius

- 273

State the relationship between kinetic energy and temperature in gases

‘The temperature of a gas (in Kelvins) is proportional to the average kinetic energy of its molecules.’

State the relationship between volume and pressure at constant temperature

(Boyle’s Law)

when the volume of gas is reduced, pressure increases, because the gas molecules hit the walls of the container more often.

p1 x v1= p2 x v2

State the relationship between pressure and kelvin temperature at constant volume

temperature and pressure are proportional

p1/T1 = p2/T2