For the given reaction: $H_{2(g)} + S_{(s)} \to H_2S_{(g)}$; $\Delta H_r = 100\, kJ/mol$ and $\Delta S_r = 400\, J/mol\cdot K$. The temperature at which the above reaction occurs reversibly is (Assuming $\Delta H_r$ and $\Delta S_r$ are independent of temperature) ..... $K$.

Gibbs free energy $G$,enthalpy $H$ and entropy $S$ are interrelated as in

Spontaneity of a chemical reaction is decided by the negative change in

For a process occurring at constant temperature and pressure,which of the following is true at equilibrium?

$\Delta G$ is net energy available to do useful work and is thus a measure of "free energy". Show mathematically that $\Delta G$ is a measure of free energy. Find the unit of $\Delta G$. If a reaction has positive enthalpy change and positive entropy change,under what condition will the reaction be spontaneous?

If $\Delta H > 0$ and $\Delta S > 0$,the reaction can proceed spontaneously at: