One mole of liquid benzene boils at its boiling point, 353.2 K, under a constant pressure of 1 bar. The enthalpy of vaporisation is 30.8 kJ mol⁻¹. Treat the vapour as an ideal gas and neglect the volume of the liquid. With w the work done on the system (R = 8.314 J K⁻¹ mol⁻¹), which pair of values is correct?

ChemistryHardHigh School (11–12)Chemical Thermodynamics › Systems, Work, Heat and the First Law JEE Main JEE Advanced

One mole of liquid benzene boils at its boiling point, $353.2\ \text{K}$ , under a constant pressure of $1\ \text{bar}$ . The enthalpy of vaporisation is $30.8\ \text{kJ mol}^{-1}$ . Treat the vapour as an ideal gas and neglect the volume of the liquid. With $w$ the work done on the system ( $R = 8.314\ \text{J K}^{-1}\ \text{mol}^{-1}$ ), which pair of values is correct?

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