Asked by stefani
Suppose 1.500 g of a compound is dissolved in 35.00 g of camphor. The freezing point of pure camphor is 178.75 °C, the freezing point of the solution is 164.4 °C and Kf(camphor) = 37.7 °C*kg/mol. Assume this compound does not dissociate. What is the molecular mass of the compound? (In g/mol, do not include units)
Answers
Answered by
DrBob222
dT = i*Kf*m
you know dT = 178.75 - 164.4 = ?
You know i = 1
You know Kf
Substitute and solve for m.
Then m = mols/kg solvent. You know kg solvent and m, solve for mols.
Then mols = grams/molar mass. You know grams and mols, solve for molar mass.
Post your work if you get stuck.
you know dT = 178.75 - 164.4 = ?
You know i = 1
You know Kf
Substitute and solve for m.
Then m = mols/kg solvent. You know kg solvent and m, solve for mols.
Then mols = grams/molar mass. You know grams and mols, solve for molar mass.
Post your work if you get stuck.
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.