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 $J$)

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

If the enthalpy and entropy change for a reaction at $298 \ K$ are $-145 \ kJ \ mol^{-1}$ and $-650 \ J \ K^{-1} \ mol^{-1}$ respectively,which one of the following statements is correct?

$A$ process has $\Delta H = 200 \ J \ mol^{-1}$ and $\Delta S = 40 \ J \ K^{-1} \ mol^{-1}$. Choose the minimum temperature above which the process will be spontaneous.

For a spontaneous process,which of the following conditions must be met?

The value of ${\left[ {\frac{dG}{dT}} \right]_P}$ is ....