A: 307 K the vapor pressure of pure 2-butanone(CH,COcH,CHy) r butanone with 48.9
ID: 717755 • Letter: A
Question
A: 307 K the vapor pressure of pure 2-butanone(CH,COcH,CHy) r butanone with 48.9 g of acetone gives a solution that is nearly ideal. HCH) s 1. m Mixing 46-4 gof2. (a) Calculate the mole fraction of 2-butanone in the solution X2-butanene in solution (b) Calculate the total vapor pressure of the solution at 307 K Total vapor pressure solution- atm (c) Calculate the mole fraction of 2-butanone in the vapor in equilibrium with the solution. X2-butanone in vapor- Submit Answer 5 question atempts remaininoExplanation / Answer
Part a
Moles of 2-butanone = mass/molecular weight
= (46.4g) / (72.11 g/mol)
= 0.6435 mol
Moles of acetone = mass/molecular weight
= (48.9g) / (58.08 g/mol)
= 0.8419
Total Moles = 0.6435 + 0.8419
= 1.4854 mol
Mol fraction of 2-butanone = Moles of 2-butanone/total moles
= 0.6435/1.4854
= 0.433
Part b
From Raoult’s law
Total vapor pressure
P =( mol fraction x vapor pressure) of 2-butanone + ( mol fraction x vapor pressure) of acetone
= 0.433 x 0.190 + (1-0.433) x 0.383
= 0.08227 + 0.217161
P = 0.2994 atm
Part c
Mol fraction of 2-butanone in vapor x P = ( mol fraction x vapor pressure) of 2-butanone
Mol fraction of 2-butanone in vapor = 0.433 x 0.190 / 0.2994
= 0.275