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Q.

∆H (vap) for water is 40.7 KJ mol^-1. The entropy of vapourisation of water is

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a

$109 J {mol}^{- 1} K^{- 1}$

b

$40.7 J {mol}^{- 1} K^{- 1}$

c

$40.7 {kJmol}^{- 1} K^{- 1}$

d

$109 {kJmol}^{- 1} K^{- 1}$

answer is B.

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Detailed Solution

$\begin{aligned} ΔS & = ΔH / T = 40.7 X 1000 J {mole}^{- 1 / 373 K} \\ = 109 J {mol}^{- 1} k^{- 1} \end{aligned}$

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