This document summarizes the states of matter and gas laws. It describes the key properties of solids, liquids, and gases. Solids have a definite shape and volume, liquids have a definite volume but no shape, and gases have no definite shape or volume. It then explains several gas laws including Boyle's Law relating pressure and volume at constant temperature, Charles' Law relating volume and temperature at constant pressure, and Avogadro's Law relating volume and number of moles of gas at constant temperature and pressure. Mathematical representations of each law are provided.
2. Solids
• Solids have definite shape and volume.
• Particles only vibrate about their fixed positions.
3. Liquids
• Intermolecular forces are intermediate of solid and gaseous state.
• Liquids have definite volume but no definite shape.
• Liquids take the shape of the container in which they are kept.
4. Gases
• Intermolecular forces are minimum.
• Particles move randomly at very high velocities.
• Gases have no definite shape or volume.
5. Gas Laws
• Gas laws are the experimentally discovered relationships
between measurable properties of gases.
• These measurable properties are pressure, volume,
temperature and mass.
6. Boyle’s Law
• Boyle’s law states that:
At constant temperature, the pressure of a fixed
amount of a gas is inversely proportional to its
volume.
8. Charles Law
• At constant pressure, the volume of a fixed mass of a gas is
directly proportional to its absolute temperature.
Mathematically,
V α T(at constant T and n).
V= kT
𝑉
𝑇
= k where k is a constant.
9. Avogadro law
• Equal volumes of all gases at same temperature and pressure
contain equal number of molecules.
• Mathematically,
Vα n (t constant p and T)
V=kn (n=number of moles of gas).
𝑉/n= k
