Question

Sodium acetate spontaneously crystallizes out of a supersaturated solution upon standing or upon the addition of a seed crystal. Which of the following is true for the thermodynamic quantities of this system for thisprocess?(a)ΔS < 0J/K, ΔH < 0 J(b)ΔS < 0J/K, ΔH > 0 J(c)ΔS > 0J/K, ΔH < 0J(d)ΔS > 0J/K, ΔH > 0J

Answer 1

Answer:

Option (c) is correct.

Explanation:

According to 2nd law of thermodynamics, every spontaneous process is associated with increase in entropy ($\Delta S>0$).

As sodium acetate crystallizes out spontaneously therefore it is associated with $\Delta S>0$.

During crystallization, bond formation takes place which results evolution of heat. In other words, crystallization phenomenon is exothermic ($\Delta H$).

So, the given crystallization process renders the following thermodynamic quantities- $\Delta S>0$ J/K and $\Delta H$ J

Option (c) is correct.