The enthalpy and entropy change for the reaction $Br_{2(l)} + Cl_{2(g)} \rightarrow 2BrCl_{(g)}$ are $30 \ kJ \ mol^{-1}$ and $105 \ J \ K^{-1} \ mol^{-1}$ respectively. The temperature at which the reaction will be in equilibrium is ............... $K$.

The correct thermodynamic conditions for a spontaneous reaction at all temperatures are:

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

For vaporization of water at $1$ atmospheric pressure,the values of $\Delta H$ and $\Delta S$ are $40.63 \ kJ \ mol^{-1}$ and $108.8 \ J \ K^{-1} \ mol^{-1},$ respectively. The temperature when Gibb's energy change $(\Delta G)$ for this transformation will be zero,is ............ $K$. (in $.4$)

For the reaction $A \to B$,$\Delta H = 4 \, kcal \, mol^{-1}$ and $\Delta S = 10 \, cal \, K^{-1} \, mol^{-1}$. At what temperature $(K)$ will the reaction become spontaneous?

What is the value of $\Delta G$ for a water system in an environment at a temperature of $100 \ K$?