How does Dalton's law of partial pressures help us with our model of ideal gases? That is, which postulates of the kinetic molecular theory dose it support?

Interpretation:

The use of Dalton’s law should be determined for the model of ideal gas and also find out the postulate of kinetic molecular theory which represents Dalton’s law.

Concept introduction: According to Dalton’s law of partial pressure, the sum of partial pressures of mixture of gases is equal to the total pressure of the gas.

Ptotal=Pgas 1+Pgas 2+Pgas 3......

The ideal gas equation is as follows:

PV=nRT

Where,

P = Pressure in atm

V = Volume in Liter

n = moles of gas

R = Ideal gas constant

T = Temperature in Kelvin.

According to Dalton’s law of partial pressure, the sum of partial pressures of mixture of gases is equal to the total pressure of the gas.

Form Dalton’s law, we can calculate the total pressure of mixture of gases present in the container. Each gas exerts separate pressure on the walls of container which is known as partial pressure of that gas. All together the gases are pressuring the container. So without calculatingtotal pressure of gases present in container, we cannot calculate the moles of any gas.

With the help of Dalton’s law and assuming that all gases present in mixture are ideal gases, we can calculate mole fraction of gas present in mixture through ideal gas equation.

The Kinetic molecular theory is based on the some simple principles and assumption which are very useful in explanation of ideal gas behaviors. This theory is composed of five postulates mentioned below:

1. There is a continuous motion along with straight line travelling in molecules of gas and a direction change observed when they colloids with other molecules and walls of the container...