If the normal boiling point of a liquid is 82 °C, what is the vapor pressure (in atm) at 50 °C? Enthalpy of vaporization = 37.2 kJ/mol K.    A. 0.61 atmB. 0.73 atmC. 0.29 atmD. 0.11 atmE. 1.0 atm

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Asked Dec 4, 2019
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If the normal boiling point of a liquid is 82 °C, what is the vapor pressure (in atm) at 50 °C? Enthalpy of vaporization = 37.2 kJ/mol K.

A. 0.61 atm
B. 0.73 atm
C. 0.29 atm
D. 0.11 atm
E. 1.0 atm

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Step 1

If the normal boiling point of a liquid is 82 °C, the vapor pressure (in atm) at 50 °C is to be calculated.

Enthalpy of vaporization = 37.2 kJ/mol K.

Step 2

Clausius-Clapeyron equation: It is used to relate the vapor pressures of a substance at two different temperatures if the enthalpy of vaporization is known.

Step 3

Given conditions are:

ΔHvap =37.2 kJ/mol.K = 37200 J/mol.K

T1 = 82°C (boiling point) = 82°C + 273 = 355 K

T2 = 50°C = 50°C +273 = 323 ...

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