The molar enthalpy of vaporisation of acetone is less than that of water. Why?

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Solution

Amount of heat required to vaporise one mole of a liquid at constant temperature and under standard pressure (1 bar ) is called its molar enthalpy of vaporisation $Δ_{v a p} H^{⊖}$ . Molar enthalpy of vaporisation of water is more than that of acetone because there is strong hydrogen bonding in $H_{2} O$ molecule.

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One mole of acetone requires less heat to vaporise than 1 mole of water. Which of the two liquids has higher enthalpy of vaporisation?

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(Δ U

1

1

100^{o} C

1

373 K = 41 k J {m o l}^{- 1}

R = 8.314 J K^{- 1} {m o l}^{- 1}

186.5 k J / m o l

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