What is Dalton's law of partial pressure?

According to Dalton's law of partial pressures, the total pressure by a mixture of gases is equal to the sum of the partial pressures of each of the constituent gases. The partial pressure is defined as the pressure each gas would exert if it alone occupied the volume of the mixture at the same temperature.

The total pressure exerted by mixture of gas is equal to the sum of the partial pressure of individual gases.

Explanation:

According to Dalton law of partial pressure,

The total pressure exerted by mixture of gas is equal to the sum of the partial pressure of individual gases.

Mathematical expression:

P (total) = P₁ + P₂ + ... P (n)

P₁ = Partial pressure of one gas

P₂ = Partial pressure of second gas

Pn = Partial pressure of number of gases

For example:

A gaseous mixture consist of He and Ne gas. The pressure exerted by He is 2 atm while neon exerted 4 atm. The total pressure will be:

P (total) = P (He) + P (Ne)

P (total) = 2 atm + 4 atm

P (total) = 6 atm