State Henry’s law. Why do gases always tend to be less soluble in liquids as the temperature is raised?
OR
State Raoult’s law for the solution containing volatile components. Write two differences between an ideal solution and a non-ideal solution.
State Henry’s law. Why do gases always tend to be less soluble in liquids as the temperature is raised?
OR
State Raoult’s law for the solution containing volatile components. Write two differences between an ideal solution and a non-ideal solution.
Henry’s law: The mass of a gas dissolved in a given volume of the liquid at constant temperature is directly proportional to the pressure of the gas present in equilibrium with the liquid. Or The solubility of a gas in a liquid at a particular temperature is directly proportional to the pressure of the gas in equilibrium with the liquid at that temperature. The dissolution of a gas in a liquid is an exothermic process, that is, it is accompanied by the evolution of heat. Thus,
Gas + Solvent ⇌ Solution + Heat
Applying Le Chatelier’s principle, the increase of temperature would shift the equilibrium in the backward direction, that is, solubility would decrease. Therefore, gases always tend to be less soluble in liquids as the temperature is raised.
OR
Raoult’s law: In a solution, the vapour pressure of a component at a given temperature is equal to the mole fraction of that component in the solution multiplied by the vapour pressure of that component in the pure state.
Ideal SolutionNon-ideal Solution1.An ideal solution of the components A and1.A non-ideal solution of the components A B is defined as the solution in which the and B is defined as the solution in which theintermolecular interactions between theintermolecular interactions between the components (A–B attractions) are of the components (A–B attractions) are of different same magnitude as the intermolecularmagnitude as the intermolecular interactionsinteractions found in the pure components found in the pure components(A–A attractions and B–B attractions).(A–A attractions and B–B attractions).2.ΔmixH=0 and ΔmixV=0.2.ΔmixH≠0 and ΔmixV≠0.
Henry’s law: The mass of a gas dissolved in a given volume of the liquid at constant temperature is directly proportional to the pressure of the gas present in equilibrium with the liquid. Or The solubility of a gas in a liquid at a particular temperature is directly proportional to the pressure of the gas in equilibrium with the liquid at that temperature. The dissolution of a gas in a liquid is an exothermic process, that is, it is accompanied by the evolution of heat. Thus,
Gas + Solvent ⇌ Solution + Heat
Applying Le Chatelier’s principle, the increase of temperature would shift the equilibrium in the backward direction, that is, solubility would decrease. Therefore, gases always tend to be less soluble in liquids as the temperature is raised.
OR
Raoult’s law: In a solution, the vapour pressure of a component at a given temperature is equal to the mole fraction of that component in the solution multiplied by the vapour pressure of that component in the pure state.
Ideal SolutionNon-ideal Solution1.An ideal solution of the components A and1.A non-ideal solution of the components A B is defined as the solution in which the and B is defined as the solution in which theintermolecular interactions between theintermolecular interactions between the components (A–B attractions) are of the components (A–B attractions) are of different same magnitude as the intermolecularmagnitude as the intermolecular interactionsinteractions found in the pure components found in the pure components(A–A attractions and B–B attractions).(A–A attractions and B–B attractions).2.ΔmixH=0 and ΔmixV=0.2.ΔmixH≠0 and ΔmixV≠0.
