How is Dalton's law of partial pressures useful in calculating the pressure of a dry gas?

300 mL of a gas A at a pressure of 600 mm is mixed with 200mL of another gas B at a pressure of 700 mm in a vessel of 2-litre capacity. What will be the total pressure of the resulting mixture, if the temperature is kept constant?

What will be the pressure of the gaseous mixture when 0.5 L of H₂ at 0.8 bar and 2.0 L of dioxygen at 0.7 bar are introduced in a 1L vessel at 27°C? 

124. A gaseous mixture containing 12g of oxygen and 52 g of nitrogen were enclosed in a vessel of 10L capacity at 27°C. Calculate:
(i) Partial pressure of each gas
(ii) Total pressure of the gaseous mixture.

A neon-dioxygen mixture contains 70.6 g dioxygen and 167·5 g neon. If pressure of the mixture of gases in the cylinder is 25 bar, what is the partial pressure of dioxygen and neon in the mixture? 

A mixture of dihydrogen and dioxygen at one bar pressure contains 20% by weight of dihydrogen. Calculate the partial pressure of dihydrogen. 

Calculate the total pressure in a mixture of 8g of dioxygen and 4g of dihydrogen confined in a vessel of 1 dm³ at 27°C. R = 0·083 bar dm³ k^–1 mol^–1. 

What do you mean by kinetic molecular theory of gases? What is its purpose?

Outline the basic assumptions/postulates of kinetic theory of gases.