Compare henry law and raoults law

Henry's law can be stated as : 
The partial pressure of a gas in vapour phase (p) is directly proportional to the mole fraction (x) of the gas in the solution at a fixed temperature.
Expressing solubility in terms of mole fraction of the gas in the solution, for a gas A and the partial pressure as p , Henry's law can be written as :
p_A = K_H x_{A    ,} where K_H is called Henry's constant.

Raoult's Law can be stated as :
For a solution of volatile liquids, the vapour pressure of a component at a given temperature is directly proportional to its mole fraction .

p₁ = p₁⁰x₁    , where p₁⁰ is the vapour pressure of pure component 1 at the same temperature.

Similarities between Raoult's law And Henry's law:
(i)Both apply to the volatile component of the solution.
(ii) Both state that the vapour pressure of any component in the solution is proportional to the mole fraction of that component in the solution.


Dissimilarities :
The two laws differ in the proportionality constant. In Raoult's law it is equal to vapour pressure of the pure component(p⁰​) while in Henry's law it is equal to an experimentally determined value of Henry's constant.