Question

question 1 (2 points)
formation of solutions where the process is endothermic can be spontaneous
provided that _______.

a) the solvent is a gas and the solute is a solid

b) they are accompanied by an increase in order

c) they are accompanied by an increase in disorder

d) they are accompanied by another process that is exothermic

question 2 (2 points)

Explanation:

For a spontaneous process, the Gibbs free energy change ($\Delta G$) must be negative. The formula is $\Delta G = \Delta H - T\Delta S$. In an endothermic process, $\Delta H$ is positive. For $\Delta G$ to be negative, $T\Delta S$ must be positive enough to overcome $\Delta H$. An increase in disorder means $\Delta S$ (entropy change) is positive. So, endothermic solution formation is spontaneous if accompanied by increased disorder (positive $\Delta S$). Option a is irrelevant to spontaneity based on phases. Option b (increase in order) means $\Delta S$ is negative, which would make $\Delta G$ more positive (non - spontaneous). Option d is incorrect as the question is about the solution formation process itself, not another process.

Answer:

c) they are accompanied by an increase in disorder