For a spontaneous change,free energy change $\Delta G$ is

The densities of graphite and diamond at $298 \, K$ are $2.25 \, g \, cm^{-3}$ and $3.31 \, g \, cm^{-3}$ respectively. If the standard free energy difference $(\Delta G^o)$ is $1895 \, J \, mol^{-1}$, the pressure at which graphite will be transformed into diamond at $298 \, K$ is:

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?

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

Which of the following formulas is correct for Gibbs free energy $(G)$?