Gibbs Energy Change — MCQ Practice

For a reaction, $\Delta H = -50 \text{ kJ/mol}$ and $\Delta S = -150 \text{ J/mol.K}$. At what temperature (in Kelvin) will the reaction become spontaneous?

Which of the following conditions will always result in a spontaneous reaction?

For a certain reaction, $\Delta G^circ = +20.0 \text{ kJ/mol}$ at $298 \text{ K}$. Calculate the equilibrium constant ($K$) for this reaction at $298 \text{ K}$. (Given: $R = 8.314 \text{ J/mol.K}$)

For the reaction $2A(g) + B(g) \rightleftharpoons 2C(g)$, $\Delta H^circ = -150 \text{ kJ}$ and $\Delta S^circ = -250 \text{ J/K}$ at $298 \text{ K}$. Calculate $\Delta G^circ$ for this reaction at $298 \text{ K}$.

Which of the following statements is INCORRECT regarding Gibbs energy change ($\Delta G$)?

For the melting of ice at $1 \text{ atm}$, which of the following is true?

If a reaction has a $\Delta G^circ = -100 \text{ kJ/mol}$ at $298 \text{ K}$, and the reaction quotient $Q = 1000$ under certain non-standard conditions at the same temperature, what can be said about the spontaneity of the reaction under these non-standard conditions? (Given: $R = 8.314 \text{ J/mol.K}$)