Test: Gas Absorption Principle

Explanation: Solute transfer from liquid to gas is known as stripping or desorption. The solute transfer of gas to liquid is known as Absorption.

Explanation: The equilibrium diagram helps to determine the flux with the help of mass transfer co-efficient and concentration gradient.

Explanation: As per the equilibrium solubility curve, if the temperature increases partial pressure increases resulting in decreasing solubility.

Explanation: Only adjacent homologous series falls in ideal solution category. Here, isobutane is an alkane and olefins are alkenes.

Explanation: Generally, Raoult’s law states that, equilibrium partial pressure of a component at certain conditions equals to the product of the mole fraction and the vapour pressure. For a pure component (i.e.) mole fraction equals one.
Therefore, the partial pressure equals vapour pressure.

Explanation: For a straight line Y=m*x, the law proved by Hendry. (i.e.) Y=(y/P) =m*x.

Explanation: Dalton proved a generalized equation states that total pressure is equals to the sum of the partial pressure of the components. Raoult’s law is applicable for only ideal solution since the partial pressure is equals to the product of mole fraction and the vapour pressure.

For a better choice of absorbent, the viscosity should be low to get the rapid absorption rates, low pressure drops in absorption tower.

Explanation: Since air won’t dissolve in water the affinity of nitrogen towards the water will be more which converts ammonia into ammonium solution. But in other options the hydrocarbons easily dissolves in polar solvents.

Explanation: Because the vapour pressure only varies linearly with compositions.

Explanation: Since air won’t dissolve in water the affinity of nitrogen towards the water will be more which converts ammonia into ammonium solution. But in other options the hydrocarbons easily dissolves in polar solvents.