The vapour pressure of two pure liquids a and b are 100 and 80 torr respectively. Total vapour pressure of solution obtained by mixing 2 moles of a and 3 moles of b would be
Answers
Answer : The total vapor pressure of the solution will be, 88 torr
Explanation : Given,
Vapor pressure of pure liquid A = 100 torr
Vapor pressure of pure liquid B = 80 torr
Moles of pure liquid A = 2 moles
Moles of pure liquid B = 3 moles
First we have to calculate the mole fraction of pure liquid A and B.
Now we have to calculate the total vapor pressure of solution.
According to the Raoult's law,
where,
= vapor pressure of solution = ?
= vapor pressure of pure liquid A
= vapor pressure of pure liquid B
= mole fraction of pure liquid A
= mole fraction of pure liquid B
Now put all the given values in the above formula, we get:
Therefore, the total vapor pressure of the solution will be, 88 torr
Answer: Total vapour pressure of solution obtained by mixing 2 moles of a and 3 moles of b would be 88 torr.
Explanation:-
According to Raoult's law, the vapor pressure of a component at a given temperature is equal to the mole fraction of that component multiplied by the vapor pressure of that component in the pure state.
and
where, x = mole fraction
= pressure in the pure state
According to Dalton's law, the total pressure is the sum of individual pressures.
,
,
The total vapor pressure is 88 torr.