Entropy — MCQ Practice

Which of the following processes will lead to an increase in the entropy of the system?

Calculate the standard entropy change ($\Delta S^\circ$) for the reaction: $2\text{SO}_2(\text{g}) + \text{O}_2(\text{g}) \rightarrow 2\text{SO}_3(\text{g})$ Given standard molar entropies ($S^\circ$) at $298\,\text{K}$: $S^\circ(\text{SO}_2(\text{g})) = 248.2\,\text{J/K·mol}$ $S^\circ(\text{O}_2(\text{g})) = 205.1\,\text{J/K·mol}$ $S^\circ(\text{SO}_3(\text{g})) = 256.8\,\text{J/K·mol}$

The enthalpy of vaporization of a liquid is $30\,\text{kJ/mol}$ and its boiling point is $300\,\text{K}$. Calculate the entropy change for the vaporization of 1 mole of the liquid.

According to the Second Law of Thermodynamics, for a spontaneous process, which of the following statements is true?

Which of the following factors would generally lead to a decrease in the entropy of a system?

According to the Third Law of Thermodynamics, what is the entropy of a perfect crystalline substance at absolute zero?