List of top Chemistry Questions on Gibbs Free Energy asked in MHT CET

Calculate \(△G^{\circ}\) for reaction,
\(\text{CH}_{4(g)}+\text{H}_{2(g)}\rightarrow \text{C}_2\text{H}_{6(g)}\) (\(K_p = 2\times 10^{17}\), \(R = 8.314 \text{JK}^{-1}\text{mol}^{-1}\))

Calculate standard Gibbs energy for any gaseous reaction if values of \(K_p\) and \(R\) respectively are \(3.5\times 10^{17}\) ; \(8.314\,\text{JK}^{-1}\text{mol}^{-1}\)

Identify from following, the relation between standard free energy change in a reaction and equilibrium constant \(K_c\).

For a certain reaction, \(\Delta \text{H}^{\circ} = 40 \text{kJ}\) and \(\Delta \text{S}^{\circ} = 80 \text{JK}^{-1}\). Find the temperature so that \(\Delta \text{G}^{\circ} = 0\)

For a certain reaction, \(\Delta H^0\) is \(-345\) kJ and \(\Delta S^0\) is \(-123 \text{JK}^{-1}\). At what temperature the change over from spontaneous to nonspontaneous will occur?

For a certain reaction \(\Delta H = -50\) kJ and \(\Delta S = -100\) J/K find the temperature so that the reaction is spontaneous.

The equilibrium constant for a reaction is \(100\). What will be the value of standard Gibbs energy change at \(298\) K ? (\(R = 8.314\) J \(\text{K}^{-1}\text{mol}^{-1}\))

For a certain reaction, $\Delta H = -210$ kJ and $\Delta S = -150$ J K$^{-1}$. Find the temperature so that $\Delta G = 0$.

Calculate $\Delta S_{\text{total}$ for a certain reaction if $\Delta H=-150\text{ kJ}$ and $\Delta S=32\text{ J K}^{-1}$ at 300 K.