InterviewSolution
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InterviewSolution
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Calculate the entropy change for the conservation of following: (a) `1g` ice to water at `273K , DeltaH_f` for `ice=6.025kJmol^(-1)`. (b) `36g` water to vapour at `373K, DeltaH_v`for `H_2O=40.63kJmol(-1)` |
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Answer» `DeltaS_("fusion")=(DeltaH_(f))/T=(6.025xx10^(3))/273` `=22.1 JK^(-1) mol^(-1)` Now, `18 g` ice melts showing a change in entropy =`22.1` `:. 1 g` ice melts showing a change in entropy `22.1/18xx1=1.227 JK^(-1)` (b) `DeltaS_(V)=(DeltaH_(V))/T=(40.63xx10^(3))/373` `=108.9 KJ^(-1)mol^(-1)` `18 g H_(2)O` vaporises to show a change in entropy `=108.9` `:. 36 g H_(2)O` vaporises to show a change in entropy `=(108.9xx36)/18=217.85 JK^(-1)` |
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