A: 307 K the vapor pressure of pure 2-butanone(CH,COcH,CHy) r butanone with 48.9

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 remainino

Explanation / 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

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