The following information is given for benzene, C6H6, at 1atm: boiling point = 80.1 °C Hvap(80.1 °C) = 30.7 kJ/mol specific heat liquid = 1.74 J/g°C At a pressure of 1 atm, what is H in kJ for the process of condensing a 24.8 g sample of gaseous benzene at its normal boiling point of 80.1 °C. kJ

The heat required for the process is 4.24 kJ

Explanation:

To calculate the number of moles, we use the equation:

Given mass of benzene = 24.8 g

Molar mass of benzene = 78.11 g/mol

Putting values in above equation, we get:

To calculate the enthalpy change of the reaction, we use the equation:

where,

= amount of heat absorbed = ?

n = number of moles = 0.318 moles

= enthalpy change of the reaction  = 30.7 kJ/mol

Putting values in above equation, we get:

Hence, the heat required for the process is 4.24 kJ

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