Assertion:A cook cries more in cutting onion rather than cutting an onion taken out from refrigerator .
Reason:The cold onion has lower vapour pressure of its volatile content.

Cutting onions taken from the fridge is more comfortable than cutting those lying a room temperture. Explain why.

Cutting onions taken from the fridge is more comfortable than cutting those lying a room temperture. Explain why.

Cutting onions taken from the fridge is more comfortable than cutting those lying a room temperture. Explain why.

Assertion : Sea water boils at higher temperature than distilled water Reason : Addition of non volatile solute to a solvent lowers the vapour pressure

Assertion (A): Vapour pressure of 0.5 M sugar solution is more than 0.5 M KCl solution. Reason (R): Relative lowering of vapour pressure is directly proportional to the number of species present in the solution.

Assertion : Vapour pressure of 0.5M sugar solution is more than 0.5M KCl solution Reason: Lowering of vapour pressure is directly proportional to the number of particles present in the solution

Assertion : The boiling point of chloroform-acetone solution is larger than expected from ideal behaviour. Reason : The forces of attraction between unlike molecules are stronger than those between like molecules in the solution. This results in lower vapour pressure as compared to an ideal solution which is responsible for the higher boiling point.

Addition of non-volatile solute to solvent lowers its vapoure pressure. Therefore, the vapour pressure of a solution (i.e, V.P. of solvent in a solution) is lower than that of pure solvent in a solution) is lower than that of pure solvent, at the same temperature. A higher temperature is needed to raise the vapour pressure upto one atmosphere pressure, when boiling point is attined. However, increase in b.pt. is small . for example, 0.1 molal aqueous sucrose solution boils at 10.05^(@)C Sea water, an aqueous solution, which is rich in Na^(+) and Cl^(-) ions, freezes about 1^(@)C lower than frozen water . At the freezing point of a pure-solvent, the reates at which two molecule stick together to form the solid and leave it to return to liquid are equal when solute is present. Few solvent molecules are in contact with surface of solid. However, the rate at which the solvent molecules leave, surface of solid remains unchanged. That is why, temperature is lowered to restore the equalibrium. The freezing depression in a dilute solution is proportional to molality of the solute. The amount of ice seperated out on cooling a solution containing 50g ethylene glycol in 200g water to -9.3^(@)C is : [ K_(f) for H_(2)O = 1.86 K "molality"^(-1) ]