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 answered this below.
i still don't get it sir
What exactly do you not understand.
XH2O = 19.6/23.8 = 0.824
Then 0.824 + XCH4N2O = 1
XCH4N2O = 1-0.823 = ?
You may be confused by where did I get the one. The sum of the mole fractions in EVERY solution must add up to 1.
Remember 100% is all of something and that is 1 when converted to a fraction so all fractions in a solution must add to 1.
To determine the mole fraction of CH4N2O in the solution, you can use Raoult's Law, which states that the vapor pressure of a solvent above a solution (P(solution)) is equal to the product of the mole fraction of the solute (X(CH4N2O)) and the vapor pressure of the pure solvent (P0).
Here's the equation:
P(solution) = X(CH4N2O) * P0
Rearrange the equation to solve for X(CH4N2O):
X(CH4N2O) = P(solution) / P0
Given:
P(solution) = 19.6 torr
P0 = 23.8 torr
Substitute the values into the equation:
X(CH4N2O) = 19.6 torr / 23.8 torr
Calculate the mole fraction:
X(CH4N2O) ≈ 0.8235
Therefore, the mole fraction of CH4N2O in the solution is approximately 0.8235.