Use data from Appendix IIB to calculate ΔS°_rxn for each of the reactions. In each case, try to rationalize the sign of ΔS°_rxn. c. CO(g) + H₂O(g) → H₂(g) + CO₂(g)

Key Concepts

Entropy (ΔS)

Entropy, denoted as ΔS, is a measure of the disorder or randomness in a system. In chemical reactions, it reflects the number of ways the molecules can be arranged. A positive ΔS indicates an increase in disorder, while a negative ΔS suggests a decrease. Understanding how the states of reactants and products influence entropy is crucial for predicting the sign of ΔS°rxn.

Standard Entropy (S°)

Standard entropy (S°) refers to the absolute entropy of a substance at standard conditions (1 bar and 25°C). Each substance has a specific standard entropy value, which can be found in thermodynamic tables. To calculate ΔS°rxn, the standard entropies of products are subtracted from those of reactants. This concept is essential for quantifying the change in disorder during a reaction.

Reaction Direction and Entropy Change

The direction of a chemical reaction and the associated entropy change can often be rationalized by considering the states of the reactants and products. In the given reaction, the conversion of gaseous reactants to gaseous products can lead to an increase in the number of moles of gas, which typically results in a positive ΔS°rxn. Analyzing the molecular complexity and the number of gas molecules helps in predicting the sign of the entropy change.