If enthalpy of vaporisation of water is $186.5 k J / m o l$ , the entropy of its vaporisation will be:

0.5

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1.0

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1.5

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Solution

The correct option is D $0.5$
Since, for any reaction, the entropy is given by,

$E n t r o p y = \frac{Δ H_{p r o c e s s}}{T e m p e r a t u r e (in Kelvin)}$

Boiling point of water = $100^{0} C$ $+ 273 K$ = $373 K$

hence, $e n t r o p y = \frac{186.5}{373} = 0.5$ (Since, vaporisation occurs at 100*C = 373K)
Hence, answer is option $A$ .

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