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
9 answers
i need help
psoln = XH2OPoH2O
Then XH2O + XCH4N2O = 1.
Solve for XCH4N2O
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
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.
Then convert to XCH4N2O.
After you have XH2O, then use the next equation,
XH2O + XCH4N2O = 1
0.824 + X = 1
Solve for X.
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?
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?
2 answers