Consider the freezing of liquid water at -10°C. For this process what are the signs for$\Delta$H, $\Delta$S, and $\Delta$G, respectively?

Question

Quizplus · Accepted Answer

The freezing of liquid water is an exothermic process, meaning that heat is released to the surroundings. Therefore, F1F1F10H is negative. The entropy of the system decreases upon freezing, so F1F1F10S is negative. The Gibbs free energy of the system decreases upon freezing, so F1F1F10G is negative.

Consider the Freezing of Liquid Water at -10°C Δ\DeltaΔ H Δ\DeltaΔ S, And

Consider the Freezing of Liquid Water at -10°C $\Delta$ H $\Delta$ S, And