a solution of CH4N2O in water has a vapor pressure of 19.6 torr. at 25C. what is the mole fraction of CH4N2O in this solution? HELP ME

WATER PURE PRESSURE (P0) IS 23.8 TORR

VAPOR PRESSURE IS 19.6 TORR
DONT KNOW HOW TO SOLVE IT ?

P(SOLUTION)= X (CH4N2O) WATER (PURE PRESSUR

i need help now

Answered above.

To find the mole fraction of CH4N2O in the solution, we need to use Raoult's law, which states that the partial pressure of a component in a solution is equal to the vapor pressure of the pure component multiplied by its mole fraction in the solution.

In this case, the vapor pressure of the pure water (P°) is given as 23.8 torr.
The vapor pressure of the solution (P(solution)) is given as 19.6 torr.
We need to find the mole fraction of CH4N2O (X(CH4N2O)).

Using Raoult's law, we can write the equation:

P(solution) = X(CH4N2O) * P°(water)

Rearranging the equation to solve for X(CH4N2O):

X(CH4N2O) = P(solution) / P°(water)

Plugging in the given values:

X(CH4N2O) = 19.6 torr / 23.8 torr

Calculating the result:

X(CH4N2O) ≈ 0.82

Therefore, the mole fraction of CH4N2O in the solution is approximately 0.82.