According to daltons law partial pressure of gas A = mole fraction of A multiplied by total pressure similarly in roults law total pressure = mole fraction of A×partial pressure of a + mole fraction of B× partial pressure of b why in all these law we are considering mole fraction and why not moles, like we can also write in roults law total pressure= moles of A× partial pressure of A + moles of B × partial pressure of B. pls explain
Solution:
While considering a binary solution of two volatile liquids in a closed vessel, both the components would evaporate and eventually an equilibrium is established between the liquid phase and the vapour phase. The partial vapour pressure of these solutions is related to the mole fraction of the two components.
French chemist Raoult gave a quantitative relationship between them. This relationship is known as Raoult's law which states that for volatile liquids the partial vapour pressure of each component in the solution is directly proportional to its mole fraction.