(a) Explain the following phenomena with the help of Henry's law.
(i) Painful condition known as bends.
(ii) Feeling of weakness and discomfort in breating at high altitude.
(b) Why soda water bottle kept at room temperature fizzes on opening?

Explain the following phenomena with the help of Henry's law Painful condition known as bends.

Explain the following phenomena with the help of Henry's law Feeling of weakness and discomfort in breaking at high altitude.

i) State Henry's law. ii) Soda water bottles are sealed under high pressure. Give reason.

(a) Explain the following : (i) Henry's law about dissolution of a gas in a liquid (ii) Boiling point elevation constant for a solvent (b) A solution of glycerol (C_(3)H_(8)O_(3)) in water was prepared by dissolving some glycerol in 500 g of water . This solution has a boiling point of 100.42 ^(@)C . what mass of glycerol was dissolved to make this solution ? ( K_(b) for water = 0.512 K kg mol^(-1) )

Read the passage given below and answer the following questions : Scuba apparatus includes a tank of compressed air toted by the diver on his or her back, a hose for carrying air to a mouthpiece, a face mask that covers the eyes and nose, regulators that control air flow, and gauges that indicate depth and how much air remains in the tank. A diver who stays down too Iong swims too deep or comes up too fast can end up with a condition called 'the bends." In this case, bubbles of gas in the blood can cause intense pain, even death. In these following questions a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices Assertion : Soft drinks and soda water bottles are sealed under high pressure. Reason : High pressure maintains the taste and texture of the soft drinks.

When a liquid is completely miscible with another liquid, a homogeneous solution consisting of a single phase is formed. If such a solution is placed in a closed evacuated vessel, the total pressure exerted by the vapour, after the system attained equilibrium will be equal to the sum of partial pressures of the constituents. A solution is said to be ideal if its constituents follow Raoult's law under all conditions of concentrations, i.e., where p_(i) is the partial pressures of the constituent i, whose mole fraction in the solution is x_(i) and p_(i)^(@) is the corresponding vapour pressure of the pure constituent. The change in the thermodynamic functions when an ideal solution is formed by mixing pure components is given by the following expression. Delta_(mix) = G = n_("total") RT sum_(i) x_(i) In x_(i) ...(i) where, n_("total") is the total amount of all the constituents present in the solution. Delta_(mix)F =- n_("total") R sum_(i) x_(i) In x_(i) ......(ii) Delta_(mix)H =- n_("total") RT sum_(i) x_(i) In x_(i) - n_("total") R sum_(i) x_(i) In x_(i) = 0 ........(iii) Delta_(mix) U = 0 .........(iv) Since botli the components of an ideal binary system follow Raoult's law of the entire range of the compositions, the partial pressure exerted by the vapours of these constituents over the solution will be given by p_(A) = x_(A) p_(A)^(@) ..........(v) p_(B) = x_(B) p_(B)^(@) .........(vi) where, x_(A) and x_(B) are the mole fractions of the two constituents in the liquid phase and p_(A)^(@) and p_(B)^(@) are the respective vapour pressure of the pure constituents. The total pressure (p) over the solution will be the sum of the partial pressure. The composition of the vapour phase (y_(A)) can be determined with the help of Dalton's law of partial pressures. Two liquids A and B form an ideal solution at temperature T. when the total vapour pressure above the solution is 600 torr, the mole fraction of A in the vapour phase is 0.35 and in the liquid phase 0.70. The vapour pressure of pure B and A are: