Question

(a) Which has greater entropy, liquid water at $\mathbf{0}\mathbf{°}\mathit{C}$or ice at$\mathbf{0}\mathbf{°}\mathit{C}$?
(b) How does the entropy of ice at$\mathbf{-}\mathbf{5}\mathbf{°}\mathit{C}$ differ, if at all, from its
entropyat$\mathbf{-}\mathbf{50}\mathbf{°}\mathit{C}$?

Short answer

(a). when the ice melts, the entropy will increase.

(b). if the total energy of the system increases, the entropy will increase.

Step-by-step solution

Introduction

Entropy is founded on the idea that everything in nature tends to shift from order to disorder in an isolated system. In matter, it is a state of unpredictability. The energy of gas particles is higher than that of solid or liquid particles. Because gas particles can move at random, they have higher entropy than liquids and solids.

Explanation of greater entropy in solution (a)

In solution (a),$0°C$ At, the water molecules in ice form an organised crystalline structure by interconnecting. The molecules in liquid water at,$0°C$ on the other hand, would be randomly organised by hydrogen bonds. Liquid water has greater entropy than ice. This is due to the fact that freezing water to ice is an exothermicreaction in which heat energy is released. As the environment becomes warmer, more energy is gained, and entropy decreases. As a result, as the ice melts, the entropy rises.

Entropy of ice differs in solution (b)

In solution (b), At high temperature, the total energy of the system increases, and thus entropy increases with risingintemperature. Ice at $-50°C$would have lower entropy than ice at -5°C because of the highly ordered structureof ice at low temperature.

Conclusion

Therefore, the energy of gas particles is higher than that of solid or liquid particles. Because gas particles can move at random, they have higher entropy than liquids and solids. It changes when the temperature changes.