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The enthalpy of vaporization of chlorofo...

The enthalpy of vaporization of chloroform is `29.4 kJmol^(-1)` at its normal boiling point of `61.7^(@)` C. What is the entropy of condensation of chlorofom at this temperature?

A

`-57.3 `R

B

`-10.6` R

C

`-1.18` R

D

10.6 R

Text Solution

Verified by Experts

The correct Answer is:
B
`Delta_("vap")H^(@) = 29.4 kJ mol^(-1)` and `T_("boiling") = 334.7` K
`Delta_("vap")H^(@) = 29.4 kJ mol^(-1)` and `T_("boiling") = 334.7` K
`rArr Delta_("vap")S^(@) = (Delta_("vap")H^(@))/(T_("boiling")) = 87.84 Jmol^(-1) K^(-1) = 10.6 R`
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