Predict which member of each of the following pairs has the greater standard entropy at 25°C: (a) Sc(s) or Sc(g). Use Appendix C to find the standard entropy of each substance. (b) NH3(g) or NH3(aq). Use Appendix C to find the standard entropy of each substance. (c) O2(g) or O3(g). Use Appendix C to find the standard entropy of each substance. (d) C(graphite) or C(diamond). Use Appendix C to find the standard entropy of each substance.

Verified step by step guidance

1. Step 1: Understand the concept of standard entropy. Standard entropy is a measure of the amount of disorder or randomness in a system. Generally, gases have higher entropy than liquids, and liquids have higher entropy than solids due to the increased freedom of movement of particles.
2. Step 2: For part (a), compare Sc(s) and Sc(g). Recognize that the gaseous state (Sc(g)) typically has a higher entropy than the solid state (Sc(s)) because gas particles are more disordered and have more freedom of movement.
3. Step 3: For part (b), compare NH3(g) and NH3(aq). Consider that gases usually have higher entropy than aqueous solutions because gas molecules are more dispersed and have more freedom to move compared to when they are dissolved in water.
4. Step 4: For part (c), compare O2(g) and O3(g). Note that molecules with more atoms generally have higher entropy due to the increased number of ways they can arrange themselves. Therefore, O3(g) might have a higher entropy than O2(g) because it has more atoms.
5. Step 5: For part (d), compare C(graphite) and C(diamond). Recognize that graphite has a layered structure allowing more freedom of movement compared to the rigid, tightly bonded structure of diamond, suggesting that C(graphite) has a higher entropy than C(diamond).