For a process to occur spontaneously,
- Aonly the entropy of the system must increase
- Bonly the entropy of the surroundings must increase
- Ceither the entropy of the system or that of the surroundings must increase
- Dthe total entropy of the system and the surroundings must increase
Explore More
Similar Questions
If the enthalpy change for the following reaction at $300 \ K$ is $+7 \ kJ \ mol^{-1}$,find the entropy change of the surrounding (in $J \ K^{-1}$)?
$H_2O_{(s)} \longrightarrow H_2O_{(l)}$
$H_2O_{(s)} \longrightarrow H_2O_{(l)}$
Among the following processes,for which process is the change in entropy $(\Delta S)$ negative?
The enthalpy of vaporization of benzene is $30.779 \ kJ/mol$ and its boiling point is $353 \ K$. Find the change in entropy for the conversion of liquid benzene to its vapour at that temperature.
Medium
View Solution$3$ moles of water is boiled at $373 \ K$ and is changed to vapour state having the same temperature. What will be the change in entropy of the system (in $kJ/K$)? [ The molar heat of vaporization of water is $40.668 \ kJ/mol$ ]
Medium
View SolutionFor an endothermic reaction $A \rightarrow B$ to occur spontaneously at a constant temperature $T$,the entropy change $\Delta S$ must be:
Easy
View SolutionVedclass Products
For Students
Vedclass Test Series
Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.
Start Free TrialFor Teachers
Exam Paper Generator
Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.
Try FreeFor Institutes
Online Exam Module
Live online exams with unlimited students, 360° analytics & white-label branding.
See Demo