Ncert Exercises & Solutions

The enthalpy of vaporisation of ${CCl}_{4}$ is $30.5 kJ {mol}^{- 1}$ . Calculate the heat required for the vaporisation of 284 g of ${CCl}_{4}$ at constant pressure.
(Molar mass of ${CCl}_{4} = 154 g {mol}^{- 1}$ )

Given that,

1 mol of {CCl}_{4} = 154 g

∆_{vap} H for 154 g {CCl}_{4} = 30.5 kJ

∴ ∆_{vap} H for 284 g {CCl}_{4} = \frac{30.5 \times 284}{154} kJ = 56.25 kJ

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