Question

using kinetic theory of gases, deduce boyles law , chaeles law, gay lussacs law and avogadros law?

Answer 1

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RANK IMPROVEMENT GUARANTEE00Using kinetic theory of gases, deduce (i) Boyle's Law (ii) Charles Law (iii) Gay Lussac's Law (iv) Avogadro's Law

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keziaadidela asked5months agoPOST ANSWER00

Hi,

Here is the answer to your question:

 41.1

 Boyle's Law states that the pressure and volume of a confined gas are inversely proportional to each other. This means that when one of the above variables increases, the other one decreases proportionately. To explain that behavior, we need to consider the kinetic molecular theory which states that molecules of a gas are in constant straight-line motion, and collide with each other and the walls of the container elastically. Gases are different from solid and liquid in that their molecules are very far apart compared to the size of molecules themselves. In fact, the volume of a gas is due to the empty space between the molecules, not the volume of molecules themselves which is negligible. When pressure is applied to a sample of a gas, molecules simply move closer to one another causing the volume to shrink. The pressure that gas exerts on the walls of its container is caused by the bombardment of molecules per unit area. When pressure is applied to the walls of a flexible container (such as a balloon), the gas molecules inside move closer together and bump into the walls of the container more often. That in turn increases the pressure of the gas in the balloon proportionately. For example, when the volume of a 2 Liter balloon filled with a gas at 1 atmosphere of pressure is reduced to 1 Liter by applying an outside pressure, the pressure of the gas inside the balloon will increase to 2 atmospheres. 41.2Answer:

Kinetic theory explains why the volume of a container must expand when the temperature of the gas inside increases in order for the pressure to remain constant.

Explanation:

Charles' law: for a fixed mass of gas at constant pressure the volume is directly proportional to the temperature.

Analysis of a gas when its temperature increases according to kinetic theory:

The temperature has increased therefore the molecules have more kinetic energy, so they move with a greater velocity.¹If the container's dimensions do not change the molecules will travel across the container between the walls in less time (because they are moving faster and covering the same distance between the container walls). This will increase the rate of collisions, which would increase the pressure.²But if the dimensions of the container increased then the molecules would cover a larger distance faster thereby maintaining a constant rate of collisions. This would maintain a constant pressure.