The entropy change for the conversion of $1 \, \text{mol}$ of liquid water to steam at $373 \, K$ is ...... $J/K$ (Given: $\Delta H_{\text{vap}} = 2.257 \, kJ/g$). (in $0.9$)
- A$105$
- B$107$
- C$108$
- D$109$
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For which one of the following reactions, the entropy change is positive?
$\Delta S_{surr}$ for an exothermic reaction is
The condition for a spontaneous process is ......
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View SolutionIce at $-5^{\circ} C$ is heated to become vapor with a temperature of $110^{\circ} C$ at atmospheric pressure. The entropy change associated with this process can be obtained from:
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View SolutionIn a reversible adiabatic process $\Delta S$ is :-
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