Calculate the Gibbs energy change for a reaction having $\Delta H = 31400 \ J$ and $\Delta S = 32 \ J \ K^{-1}$ at $1000^{\circ} C$. (in $J$)

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 $.4$)

An enthalpy diagram for a particular reaction is given in the figure. Is it possible to decide the spontaneity of a reaction from the given diagram? Explain.

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

$A$ minus sign of the free energy change denotes that

Which of the following set of thermodynamic conditions is true for the reaction to be spontaneous at high temperature?