Question

A mixture of N2, H2 and He have mole fractions of 0.25, 0.65, and 0.10, respectively. What is the partial pressure of N2 if the total pressure of the mixture is 3.9 atm?

Answer 1

.98

Step-by-step explanation:

Answer 2

Answer: The partial pressure of
`N_2` if the total pressure of the mixture is 3.9 atm is 0.975 atm

Step-by-step 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.

`p_A=x_A* P_T`

where, x = mole fraction of nitrogen in solution = 0.25

`p_A` = partial pressure of nitrogen = ?

`P_T` = Total pressure = 3.9 atm

Putting in the values :

`p_A=0.25* 3.9=0.975atm`

The partial pressure of
`N_2` is 0.975 atm