As per second law of thermodynamics a process taken place spontaneously if and only if the entropy of the universe increases due to the process. Change in entropy is given by Delta S = (Q_(rev))/(T) A gas C_(V) = (0.2 T) Cal K^(-1) . What is the change in its entropy when one mole of it is heated from 27^(@)C to 127^(@)C at constant volume ?
4Fe(s)+3O_(2(g)) to 2Fe_2O_3(g) . The value of DeltaS is -550 JK^(-1) and the value of DH is -1650 kJ at 298 K. Does the process is spontaneous or not?
For the reaction I_(2(g)) hArr I_(2(s)), Delta H= -ve . Then choose the correct statement from the following (A) The process is spontaneous at all temperature (B) The process is accompained by an increase in entropy (C ) The process is accompained by a decrease in entropy (D) The process is accompained by a decrease in enthalpy
A process is spontaneous at all temperatures when
For a certain reaction, Delta H^(0) " & " Delta S^(0) respectively are 400kJ & 200 J/mol/K. The process is non-spontaneous at
NARENDRA AWASTHI-THERMODYNAMICS-Level 3 - Match The Column
