Question

Carbon disulfide has a vapor pressure of 363 torr at 25 °C and a normal boiling point of 46.3 °C. Find ΔHvapΔHvap for carbon disulfide.

Step 1

Clausius-Clapeyron equation signifies the relationship between heat of vaporisation and pressure at a specific temperature, labelled below as equation (1). In this equation, P_{1} represents vapor pressure at temperature T_{1}, P_{2} represents vapor pressure at temperature T_{2}, R represents universal gas constant and ΔH_{vap} represents enthalpy change of vaporisation of the substance.

Normal boiling point of a liquid is defined as a temperature at which the vapor pressure of liquid becomes equal to the pressure of gas above it (atmospheric pressure). Hence, the liquid has a pressure of 1 atm ( = 760 torr) at its normal boiling point.

Step 2

Convert the values of temperatures T_{1} and T_{2} into Kelvin units by using the above relation.

Step 3

The enthalpy of vaporisation of carbon disulf...

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