Ethanol has a normal boiling point of 78.3 degrees celcius. Why is the normal boiling point...

Ethanol has a normal boiling point of 78.3 degrees celcius. Why is the normal boiling point higher than methanol but lower than iso-propanol (Normal boiling point = 82.3, heat of vaporization = 45.4)? Would you expect the heat of vaporization of ethanol to follow the same trend? Explain.

AND

Calculate the heat of vaporixation of cyclohexane using the normal boiling point of 80.7 degrees celcius. The vapor pressure of cyclohexane at 25.0 degrees celcius is 0.132 atm.

Expert Solution

The london (dispersion) forces are stronger in methanol

The hydrogen bonds in ethanol are stronger than in methanol.

The hydrogen bonds in iso propanol are stronger than in ethanol.

ln(P2/P1) = H/R [1/T1 ---1/T2]

P2 = 0.132atm, P1 = 1atm

T1 = 80.7 + 273 = 353.7 K

T2 = 25+273 = 298K

R = 8.314joule/mole-K

ln(0.132/1) = H/8.314 [1/353.7----1/298]

-2.024*8.314 = H[0.002827--0.003355]

H =16.96 /0.000528 = 32122 joule = 32.122kj

queen_honey_blossom answered 2 years ago

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