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Q.

The boiling point of chloroform, ${CHCl}_{3}$ , is ${61.7}^{\circ} C$ and its enthalpy of vaporization is ${31.4 kJ-mol}^{- 1}$ Calculate the molar entropy of vaporization for chloroform :

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a

$509 J \times {mol}^{- 1} \cdot K^{- 1}$

b

$10.7 J \times {mol}^{- 1} \cdot K^{- 1}$

c

$93.8 J \times {mol}^{- 1} \cdot K^{- 1}$

d

$301 J \times {mol}^{- 1} \cdot K^{- 1}$

answer is B.

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Detailed Solution

Change in entropy for this case,

$Δ S = \frac{31.4 \times 10^{3}}{334.7} = 93.8 J {mol}^{- 1} K^{- 1}$

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The boiling point of chloroform, CHCl3, is 61.7∘C and its enthalpy of vaporization is 31.4 kJ-mol −1 Calculate the molar entropy of vaporization for chloroform :