For an exothermic solution process, which of the following statements is true?

• A. The process cannot occur spontaneously at any temperature.
• B. The enthalpy change of solution (ΔH_soln) is positive.
• C. The temperature of the surroundings increases as the solution forms.
• D. Energy is absorbed from the surroundings during the solution process.

Answer: (C)

Verified step by step guidance

1. Understand the meaning of an exothermic solution process: it releases heat to the surroundings, so the enthalpy change of solution (\$\Delta H_{soln}\$) is negative, not positive.
2. Recall that spontaneity depends on Gibbs free energy change (\$\Delta G = \Delta H - T\Delta S\$), so an exothermic process can be spontaneous at certain temperatures.
3. Analyze the effect on surroundings: since heat is released, the temperature of the surroundings increases as the solution forms.
4. Evaluate the incorrect statements: the process can occur spontaneously, \$\Delta H_{soln}\$ is not positive, and energy is not absorbed but released.
5. Conclude that the true statement is that the temperature of the surroundings increases during the exothermic solution process.