Enthalpy of vaporisation for water is $186.5$ KJ $m o l e^{- 1}$ . The entropy change during vaporisation is ______ KJ $m o l e^{- 1}$ .

0.5

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1.0

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Solution

The correct option is A $0.5$
We are given, $Δ H = 186.5 K J m o l^{- 1}$
Boiling point of water = $(100^{o} C + 273) K = 373 K$
Entropy Change $(Δ S) = \frac{Δ H}{T} = \frac{186.5 K J m o l e^{- 1}}{373 K} = 0.5 K J m o l^{- 1} K^{- 1}$

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Enthalpy of vaporisation for water is 186.5KJmole−1. The entropy change during vaporisation is ______ KJmole−1.

The correct option is A 0.5We are given, ΔH=186.5KJmol−1 Boiling point of water = (100oC+273)K=373KEntropy Change (ΔS)=ΔHT=186.5KJmole−1373K=0.5KJmol−1K−1

Enthalpy of vaporisation for water is $186.5$ KJ $m o l e^{- 1}$ . The entropy change during vaporisation is ______ KJ $m o l e^{- 1}$ .

The correct option is A $0.5$
We are given, $Δ H = 186.5 K J m o l^{- 1}$
Boiling point of water = $(100^{o} C + 273) K = 373 K$
Entropy Change $(Δ S) = \frac{Δ H}{T} = \frac{186.5 K J m o l e^{- 1}}{373 K} = 0.5 K J m o l^{- 1} K^{- 1}$