Gas Laws and Kinetic Molecular Frequency.

Gas Laws and Kinetic Molecular Theory

Charles' Law

The ratio of the volume and temperature of a gas is constant at a constant pressure. Since the ratio of the volume and temperature of gas is constant at a constant pressure, it remains the same at different times. 

Equation:  V₁/T₁ = V₂/T₂

 

Boyle's Law

The product of a pressure and the volume of a gas is constant at constant temperature. Since the product of the pressure and the volume of a gas is constant at constant temperature, it remains the same at different times.

Equation:  P₁V₁ = P₂V₂

 

Gay-Lussac's Law

The ratio of the pressure and temperature of a gas is constant at constant volume. Since the ration of the pressure and temperature is constant at constant volume, it remains the same at different times. 

Equation: P₁/T₁ = P₂/T₂

 

Combined Gas Law

The ratio of the product of pressure and volume to the temperature of a gas is constant. 

Equation:  P₁V₁/T₁ = P₂V₂/T₂

 

Avogadro's Law 

The ratio of the volume and mols of a gas is constant at constant temperature and pressure. 

Equation:  V₁/n₁ = V₂/n₂

 

Ideal Gas Law

The ideal gas law relates to the pressure, volume, temperature, and number of mols for a gas sample. 

Equation: PV = nRT

 

Kinetic Molecular Theory

Gas molecules are in constant motion. The gas molecules in a sample move at hundreds of miles per hour in straight line paths. Even though they are very tiny, the molecules inside the container hit each other and the walls of the container. There are so many collisions that they add up to a measurable pressure. 

Gas pressure is caused by molecules hitting the walls of the container. 

Pressure increases as the frequency of collisions increases. It also increases if the molecules hit the walls with greater force. Pressure and temperature are proportional if the volume of the gas does not change: P = kT. An increase in temperature increases both the collision frequency and the force with which the molecules hit the walls.