Asked by Emily
Calculate the vapor pressure of a solution containing 28.7g of glycerin (C3H8O3) in 136mL of water at 30.0 ∘C. The vapor pressure of pure water at this temperature is 31.8 torr. Assume that glycerin is not volatile and dissolves molecularly (i.e., it is not ionic) and use a density of 1.00 g/mL for the water.
Answers
Answered by
DrBob222
mols glycerin = grams/molar mass = ?
mols H2O = grams/molar mass = ?
mols fraction glycerin = Xgly = mols glycerin/total mols.
Then pH2O = Xglycerin*P<sup>o</sup><sub>H2O</sub>
mols H2O = grams/molar mass = ?
mols fraction glycerin = Xgly = mols glycerin/total mols.
Then pH2O = Xglycerin*P<sup>o</sup><sub>H2O</sub>
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.