Question

The normal boiling point of water is 100 c. use the Clasius-Clapeyron equation to determine the...

The normal boiling point of water is 100 c. use the Clasius-Clapeyron equation to determine the temperature (in °C) at which water will boil in the rocky mountains where atmospheric pressure is 0.657 atm. ΔHvap of water is 40.7 KJ/mole.

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Answer #1

Use the Clasius-Clapeyeron equation.

ln (P1/P2) = -ΔH/R*(1/T1 – 1/T2)

where P1 = 1.000 atm; P2 = 0.657 atm, T1 = 100⁰C = (100 + 273) K = 373 K and ΔH = 40.7 kJ/mol = (40.7 kJ/mol)*(1000 J/1 kJ) = 40700 J/mol.

Plug in values

ln (1.000 atm/0.657 atm) = -(40700 J/mol)/(8.314 J/mol.K)*(1/373 – 1/T2) K-1

===> 0.42007 = (-4895.357229 K)*(0.00268096 – 1/T2) K-1

===> 0.42007/4895.357229 = -(0.00268096 – 1/T2)

===> 8.580987*10-5 = -0.00268096 + 1/T2

===> 1/T2 = 0.00276678987

===> T2 = 1/0.00276678987 = 361.429668 ≈ 361.43

The required temperature is 361.43 K = (361.43 – 273)⁰C = 88.43⁰C (ans).

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