Asked by Pagye
A solution is made by mixing 47.0 mL of ethanol, C2H6O, and 53.0 mL of water. Assuming ideal behavior, what is the vapor pressure of the solution at 20 °C?
Answers
Answered by
DrBob222
mol fraction EtOH = XEtOH = mols EtOH/total mols.
mol fraction H2O = XH2O = mols H2O/total mols.
mols EtOH = grams/molar mass. You will need to covert mL ethanol to grams by using the density EtOH at 20C.
mols H2O = grams/molar mass. Use density of water at 20C.
pH2O = XH2O * PH2O at 20 C.
pEtOH = XEtOH * PEtOH at 20 C.
Total P = pEtOH + pH2O.
mol fraction H2O = XH2O = mols H2O/total mols.
mols EtOH = grams/molar mass. You will need to covert mL ethanol to grams by using the density EtOH at 20C.
mols H2O = grams/molar mass. Use density of water at 20C.
pH2O = XH2O * PH2O at 20 C.
pEtOH = XEtOH * PEtOH at 20 C.
Total P = pEtOH + pH2O.
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.