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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Solution

One mole of acetone requires less heat to vaporise than 1 mole of water. Hence, acetone has less enthalpy of vaporisation and water has higher enthalpy of vaporisation. It can be represented as $(Δ H_{V})$ water > $(Δ H_{V})$ acetone.

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Similar questions

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

186.5

m o l e^{- 1}

m o l e^{- 1}

H_{2 (g)} + 1 / 2 O_{2 (g)} ⟶ {H_{2} O}_{(l)}; Δ H = - 285.77 k J / m o l e

H_{2 (g)} + 1 / 2 O_{2 (g)} ⟶ {H_{2} O}_{(l)}; Δ H = - 241.84 k J / m o l e

Δ U

2.0

100^{o} C

(Δ H_{v})

100^{o} C

40 K J {K J m o l}^{- 1}

Δ E

2.0

100^{o} C

Δ H

100^{o} C

40.66 k J {m o l}^{- 1}

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