A certain process has ΔH° 0, ΔS° 0. The values of ΔH° and ΔS° do not depend on the temperature. Which of the following is a correct conclusion about this process?

Question

A certain process has ΔH° > 0, ΔS° < 0, and ΔG° > 0. The values of ΔH° and ΔS° do not depend on the temperature. Which of the following is a correct conclusion about this process?

Quizplus · Accepted Answer

Since ΔG° is always positive, the reaction is non-spontaneous at all temperatures. The negative value of ΔS° indicates that the disorder of the system decreases during the process, which makes the process less favorable. The positive value of ΔH° indicates that the process is endothermic, which requires an input of energy to proceed. If the reaction is non-spontaneous at all temperatures, it means that the energy input required to drive the reaction forward exceeds the energy output of the system.

A Certain Process Has ΔH° > 0, ΔS° < 0