Derive Dalton's law of particial pressures on the basis of kinetic theory of gases.

Define Charles' law and Dalton's law of partial pressure. How does kinetic molecular theory of gases account for these laws?

To which of the following Dalton's law of partial pressure is not applicable ?

State (i) Charles's law (ii) Dalton's law of partial pressures.

Assertion: If H_(2) and Cl enclosed separately in the same vessel exert pressure of 100 and 200 mm respectively, their mixture in the same vessel at the same temperature will exert a pressure of 300 mm Reason: Dalton's law of partial pressures states that total pressure is the sum of partial pressures.

Read the passage given below and answer the following questions : Raoult's law states that for a solution of volatile liquids, the partial vapour pressure of each component of the solution is directly proportional to its mole fraction present in solution. Dalton's law of partial pressure states that the total pressure P_("total") over the solution phase in the container will be the sum of the partial pressures of the components of the solution and is given as: P_("total") = P_1 + P_2 What type of deviation from Raoult's law does the above graph represent ?

Read the passage given below and answer the following questions : Raoult's law states that for a solution of volatile liquids, the partial vapour pressure of each component of the solution is directly proportional to its mole fraction present in solution. Dalton's law of partial pressure states that the total pressure P_("total") over the solution phase in the container will be the sum of the partial pressures of the components of the solution and is given as: P_("total") = P_1 + P_2 Which of the following aqueous solutions should have the highest boiling point ?