class: SS 2
Topic: Kinetic Molecular Theory of Gas
Kinetic Molecular Theory of Gas
If the gas volume is increased at constant temperature the molecules take longer time to bombard the wall. This fewer impacts per second is seen. The pressure of the gas thus decreased, when the gas volume is decreased, molecules take less time to travel between the piston and the wall opposite. The molecule therefore hit the walls of the container more often in unit time therefore the gas pressure increases as more impacts per second are made.
Boyle’s law states that at constant temperature, the absolute pressure and volume of a given mass of confined gas are inversely proportional.
Charles’law states that at constant pressure, the volume of a gas increases or decreases by the same factor as its temperature.
So, an increase in temperature at constant pressure would lead to an increase in the gas volume.If the gas is heated at constant pressure, the molecule gain kinetic energy and hit the walls of the container more often in a second. This leads to an increase in pressure.In order to keep the pressure constant, the volume of the containing vessle must be increased in order that the molecule would travel longer distance before striking the wall of the container.
Pressure Law or Gay Lussac’s Law
The pressure of a fixed mass of gas increases as its temperature increases at constant pressure. when the temperature of a fixed mass of gas is increased at constant volume, the average kinetic energy of the molecule increases.
1. If the volume of gas is increased at constant temperature, the _______________________
2. An increase in temperature at constant pressure would lead to ________________________