Which of the following is true for all reversible endothermic processes?

• A. The system absorbs heat from the surroundings.
• B. The system releases heat to the surroundings.
• C. The temperature of the surroundings increases.
• D. The enthalpy change (ΔH) is negative.

Answer: (A)

Verified step by step guidance

1. Understand the meaning of an endothermic process: it is a process in which the system absorbs heat from the surroundings, meaning heat flows into the system.
2. Recall that in a reversible process, the system and surroundings are in near-equilibrium at every step, so changes happen very slowly and can be reversed without net change.
3. Analyze the enthalpy change (\$\Delta H\$): for an endothermic process, \$\Delta H > 0\$, meaning the system gains heat, so \$\Delta H\$ is positive, not negative.
4. Consider the effect on the surroundings: since the system absorbs heat, the surroundings lose heat, so the temperature of the surroundings typically decreases or remains constant, not increases.
5. Conclude that the true statement for all reversible endothermic processes is that the system absorbs heat from the surroundings.