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The volume, temperature and pressure exerted by a particular gas are highly dependent on one another. This is explained by several Gas Laws. Boyle’s Law states that when the temperature is kept constant, pressure of gas is inversely proportional to the volume. Relating this principle to molar volume, the higher the pressure, the smaller the volume the gas particles occupies. When the volume of the container enclosing the gas is reduced, there are more gas particles per unit volume. The gas particles collide with each other and the wall of container with higher frequency and this will exert a higher pressure. The kinetic energy remains the same and temperature remains constant. Charles’ Law ( Law of Volume ) reveals that when pressure is kept constant, the volume of gas is directly proportional to the temperature of the gas in kelvin. Relating this back to molar volume, the higher the temperature, the higher the volume the gas occupies. When a certain amount of gas is heated to a higher temperature, the gas particles will have higher kinetic energy. This induces them to move with high speed which is associated by a higher collision rate with other particles. The volume of the gas increases so as to remain a constant pressure. Pressure Law ( Gay-Lussac’s Law ) declare that when the volume of gas is kept constant, its pressure will be directly proportional to its temperature in kelvin. When a particular gas is heated in a fixed volume of container, the gas particles will absorb the heat energy supplied and gain an increase in kinetic energy. This is associated by an increase in collision rate*…show more content…*

The graph for each law are shown below : Boyle’s Law Charles’s Law Pressure Law ( Gay-Lussac’s Law ) P1V1 = P2V2 V1 / T1 = V2 / T2 P1 / T1 = P2 / T2 Temperature constant Pressure constant Volume

The graph for each law are shown below : Boyle’s Law Charles’s Law Pressure Law ( Gay-Lussac’s Law ) P1V1 = P2V2 V1 / T1 = V2 / T2 P1 / T1 = P2 / T2 Temperature constant Pressure constant Volume

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