Find the correct statement.

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(B) According to the $2^{nd}$ Law of Thermodynamics,for any spontaneous process in an isolated system,the total entropy change $(\Delta S_{total})$ mu

Vedclass · Accepted Answer

For an irreversible spontaneous process,the entropy of an isolated system increases.

Vedclass · Answer

(B) According to the $2^{nd}$ Law of Thermodynamics,for any spontaneous process in an isolated system,the total entropy change $(\Delta S_{total})$ must be greater than zero,i.e.,$\Delta S_{total} > 0$.For an irreversible spontaneous process,the entropy of the universe (system   surroundings) increases.Specifically,for an isolated system,$\Delta S_{system} > 0$ for an irreversible spontaneous process.Option $B$ correctly states that for an irreversible spontaneous process,the entropy of an isolated system increases.

Similar Questions

The entropy change,in the conversion of one mole of liquid water at $373 \, K$ to vapour at the same temperature is (Latent heat of vaporization of water,$\Delta H_{vap} = 2.257 \, kJ/g$) ........ $J \, K^{-1}$ (in $.9$)

Identify from the following physical transformations that exhibits a decrease in entropy.

Considering entropy $(S)$ as a thermodynamic parameter,the criterion for the spontaneity of any process is

The true statement amongst the following is

At $1 \ atm$ pressure,if $\Delta S_{\text{vap}} = 75 \ J \ K^{-1} \ mol^{-1}$ and $\Delta H_{\text{vap}} = 30 \ kJ \ mol^{-1}$,what will be the boiling point of the liquid in $K$?

Vedclass Test Series

Exam Paper Generator

Online Exam Module