Question:3. State Dalton’s law of partial pressure with explanation.

Ans. : Dalton’s law of partial pressure: At constant temperature, in a mixture of gases which do not chemically react with one another, the total pressure of the mis sum of the partial pressure of the constituent gases.

Let, P be the total pressure of a gaseous mixture containing ‘n’ components gass and  f1, f2, f3……. fn . be the partial pressure of the ‘n’ components respectively. Then from this law-

P = f+  f2 +  f3  + ………… +  fn   ………………………. (i)

Explanation: Let n1, n2, and n3 moles of gases are mixed together in a container of volume V and at constant temperature, and their partial pressure P1, P2 and P3 respectively and of the total pressure mixture is P. Since n1 mole of the first gas exerts pressure P1 in volume V at temperature T, then from the ideal gas equation,

Question 4: Prove that “partial pressure = total pressure mole fraction.”

Ans.: Let n1, n2, and n3 moles of gases are mixed together in a container of volume V and at constant temperature, and their partial pressure P1, P2 and P3 respectively and of the total pressure mixture is P. Since n1 mole of the first gas exerts pressure P1 in volume V at temperature T, then from the ideal gas equation,

Partial pressure = Total pressure x mole fraction (Proved).

Or partial pressure of a gas mixture, is equal to the product of its mole fraction X total pressure of the gas mixture.

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