States of matter

Question 1

Kinetic theory of gases

Answer 1

Idea that the molecules in gases are in constant movement

Question 2

Kinetic theory assumptions

Answer 2

Gas molecules move rapidly and randomly
The distance between gas molecules is much greater than the diameter of the molecules so the volumes of the molecules is negligible
There are no forces of attraction or repulsion between the molecules
All collisions between particles are elastic (no kinetic energy lost in collisions)
The temp of the gas is related to the average kinetic energy of the molecules

Question 3

A theoretical gas that fits kinetic theory assumptions is called an

Answer 3

Ideal gas

Question 4

Real gases are

Answer 4

The actual gases we encounter

Question 5

PV=nRT

Answer 5

P= pressure (P)
V= volume (m3)
n= moles (mol)
R= gas constant (8.31)
T= temperature in K

Question 6

PV= mRT/M

Answer 6

P= pressure (P)
V= volume (m3)
m= mass (g)
R= gas constant (8.31)
T= temperature in K
M= molar mass (gmol-1)

Question 7

Vapour pressure

Answer 7

Pressure exerted by a vapour at equilibrium