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Chemical thermodynamics is the study of the interrelation of heat and work with chemical reactions or with physical changes of state within the confines of the laws of thermodynamics. It involves assessing the energy changes that occur during a process and how energy is transferred and converted.

One of the fundamental concepts in chemical thermodynamics is the first law, which states that energy cannot be created or destroyed, only transformed. Reactions that absorb energy from the surroundings are termed endothermic, while those that release energy are called exothermic. Another vital principle is the second law of thermodynamics, which introduces the concept of entropy—an important component of our current discussion.

Entropy is a measure of the disorder or randomness in a system. In chemical processes, we consider the entropy of the reactants and products to understand the direction in which a reaction is naturally inclined to proceed. The second law states that the total entropy of an isolated system can never decrease over time. This means that the entropy of the universe, which is the ultimate isolated system, tends to increase.

Entropy changes significantly during phase transitions. For instance, when a solid melts into a liquid or a liquid vaporizes into a gas, entropy increases because the molecules in the more disordered states (liquid and gas) have greater freedom of motion than in a solid.

An important rule of thumb is that, in general, the entropy of a substance increases with temperature or when a phase change occurs from solid to liquid to gas. However, it's not just about state changes; entropy can also change with chemical reactions or when a mix of substances changes its composition, as seen in the provided exercise.

In the context of chemical reactions, phase changes can have a significant influence on the system’s entropy. For instance, the production of gaseous products from solid reactants tends to lead to an entropy increase, as gas particles are more disordered than those in the solid phase. This is noticeable in the given exercise for reaction (b), where the transformation of calcium carbonate, a solid, to calcium oxide, another solid, and carbon dioxide, a gas, results in greater disorder and thus a positive entropy change.

Predicting the sign of entropy changes in chemical reactions involves assessing the disorder before and after the reaction. A reaction that results in more gas particles or a greater number of moles usually indicates an increase in entropy. In contrast, a reaction that yields fewer gas molecules or less volume will typically signify a decrease in entropy.

When we analyze the exercises provided, we can apply these concepts to predict the signs of entropy changes. For reaction (c), the entropy decreases because three moles of acetylene gas react to form only one mole of benzene gas, leading to a decrease in the system’s disorder. This illustrates well how a lessening in particle count, especially in gases, can signify a reduction in entropy.

However, it’s crucial to remember that the nature of reactants and products also matters. In reaction (d), we convert three gaseous molecules and one solid into two solids and three gases. Despite the moles of gas remaining constant, there is an overall increase in the number of particles, signifying increased disorder. Therefore, we would predict that the entropy change for reaction (d) is positive. Thus, practical experience and an understanding of molecular behavior in different states are essential in predicting entropy changes in chemical reactions.