Here are the essential concepts you must grasp in order to answer the question correctly.
Kinetic Molecular Theory
The Kinetic Molecular Theory explains the behavior of gases in terms of the motion of their particles. It posits that gas particles are in constant, random motion and that they collide with each other and the walls of their container. These collisions result in pressure, as the force exerted by the particles on the walls of the container is what we measure as gas pressure.
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Pressure Definition
Pressure is defined as the force exerted per unit area. In the context of gases, it is the result of countless collisions of gas molecules with the surfaces of their container. The greater the number of collisions and the higher the energy of the particles, the greater the pressure exerted by the gas.
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Law of Definite Proportions
Temperature and Pressure Relationship
The relationship between temperature and pressure in gases is described by Gay-Lussac's Law, which states that the pressure of a gas is directly proportional to its absolute temperature when volume is held constant. As temperature increases, gas particles move faster, leading to more frequent and forceful collisions with the container walls, thereby increasing the pressure.
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Standard Temperature and Pressure