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
psoln = XH2OPoH2O
Then XH2O + XCH4N2O = 1.
Solve for XCH4N2O
how u find mole fraction please
mole fraction of water
psoln = XH2OPoH2O
Then XH2O + XCH4N2O = 1.
Solve for XCH4N2O
im confused still
The first line is the equation you use. You know psoln = 19.6 torr and you know Po H2O is 23.8 torr. Solve for XH2O. It's as simple as 19.6/23.8 = ?
Then convert to XCH4N2O.
After you have XH2O, then use the next equation,
XH2O + XCH4N2O = 1
0.824 + X = 1
Solve for X.
i have another question.
oles in 4.9g = grams/molar mass = ?
m = molality = mols/kg solvent
delta T = Kf*m. Solve for delta T and subtract from the normal freezing point of H2O (0C) to find the new freezing point.
pi = MRT
M is molarity but in dilute solutions M and m are almost the same. R is 0.08206 and T must be in kelvin; pi comes out in atmospheres.
for this problem the answer is 1.94 not 2.02 what is wrong?
To find the mole fraction of CH4N2O in the solution, you can use Raoult's Law. Raoult's Law states that the vapor pressure of a component in an ideal solution is directly proportional to its mole fraction in the solution.
First, let's define the variables:
P(solution) = total vapor pressure of the solution
P0 = vapor pressure of pure water
P(CH4N2O) = vapor pressure of the CH4N2O component in the solution
X(CH4N2O) = mole fraction of CH4N2O
According to Raoult's Law, the vapor pressure of the solution is the sum of the partial pressures of the individual components:
P(solution) = P(CH4N2O) + P0
You know that P(solution) is 19.6 torr and P0 is 23.8 torr. Therefore, you can rearrange the equation to solve for P(CH4N2O):
P(CH4N2O) = P(solution) - P0
P(CH4N2O) = 19.6 torr - 23.8 torr
P(CH4N2O) = -4.2 torr (Note: The negative sign indicates that the CH4N2O component does not contribute to the vapor pressure)
Now, to find the mole fraction of CH4N2O, you can use the equation:
X(CH4N2O) = P(CH4N2O) / P(solution)
X(CH4N2O) = (-4.2 torr) / 19.6 torr
X(CH4N2O) = -0.214
However, mole fractions cannot be negative. In this case, it suggests that the vapor pressure of CH4N2O is lower than P0, which is not physically possible. Thus, we conclude that there might be an error in the calculation or assumption.
Please double-check your values and ensure that you have the correct data for solving this problem.