Asked by yoo
A solution contains 5.00 g of urea, CO(NH2)2 (a nonvolatile solute) and 0.100 kg of water. If the vapor
pressure of pure water at 25 °C is 23.7 torr, what is the vapor pressure of the solution assuming ideal
behavior?
pressure of pure water at 25 °C is 23.7 torr, what is the vapor pressure of the solution assuming ideal
behavior?
Answers
Answered by
DrBob222
How many moles urea? That's moles = g/molar mass.
moles urea = 5.00/molar mass urea = ?
moles H2O = 1000 g/molar mass H2O = ?
Total mols = mols urea + moles water = ?
moled fraction water X<sub>H2O</sub> = ?
P<sub>solution</sub> = X<sub>H2O</sub>*P<sup>o</sup><sub>H2O</sub>
Substitute and solve. Post your work if you get stuck.
moles urea = 5.00/molar mass urea = ?
moles H2O = 1000 g/molar mass H2O = ?
Total mols = mols urea + moles water = ?
moled fraction water X<sub>H2O</sub> = ?
P<sub>solution</sub> = X<sub>H2O</sub>*P<sup>o</sup><sub>H2O</sub>
Substitute and solve. Post your work if you get stuck.
Answered by
DrBob222
oops. Left out a step.
To get XH2O it is mols H2O/total moles = ?
To get XH2O it is mols H2O/total moles = ?
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.