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
Answered above.
To find the mole fraction of CH4N2O in the solution, you can use Raoult's law, which states that the vapor pressure of a component in a solution is equal to the product of its mole fraction in the solution and its pure vapor pressure.
The formula for Raoult's law is:
P(solution) = X(CH4N2O) * P0(CH4N2O)
Where:
P(solution) is the vapor pressure of the solution
X(CH4N2O) is the mole fraction of CH4N2O in the solution
P0(CH4N2O) is the pure vapor pressure of CH4N2O
Given that:
P(solution) = 19.6 torr
P0(CH4N2O) = 23.8 torr
We can rearrange the formula to solve for X(CH4N2O):
X(CH4N2O) = P(solution) / P0(CH4N2O)
Substituting in the given values:
X(CH4N2O) = 19.6 torr / 23.8 torr
Now, divide the numerator by the denominator:
X(CH4N2O) ≈ 0.82
Therefore, the mole fraction of CH4N2O in the solution is approximately 0.82.