Textbook Question
For a certain chemical reaction, ΔH° = -35.4 kJ and ΔS° = -85.5 J/K. (b) Does the reaction lead to an increase or decrease in the randomness or disorder of the system?
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Ch.19 - Chemical Thermodynamics
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement111
- Ch.2 - Atoms, Molecules, and Ions166
- Ch.3 - Chemical Reactions and Reaction Stoichiometry138
- Ch.4 - Reactions in Aqueous Solution127
- Ch.5 - Thermochemistry104
- Ch.6 - Electronic Structure of Atoms109
- Ch.7 - Periodic Properties of the Elements107
- Ch.8 - Basic Concepts of Chemical Bonding102
- Ch.9 - Molecular Geometry and Bonding Theories120
- Ch.10 - Gases122
- Ch.11 - Liquids and Intermolecular Forces79
- Ch.12 - Solids and Modern Materials102
- Ch.13 - Properties of Solutions99
- Ch.14 - Chemical Kinetics153
- Ch.15 - Chemical Equilibrium83
- Ch.16 - Acid-Base Equilibria109
- Ch.17 - Additional Aspects of Aqueous Equilibria117
- Ch.18 - Chemistry of the Environment60
- Ch.19 - Chemical Thermodynamics109
- Ch.20 - Electrochemistry113
- Ch.21 - Nuclear Chemistry79
- Ch.22 - Chemistry of the Nonmetals52
- Ch.23 - Transition Metals and Coordination Chemistry57
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry7
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not the one you use?Change textbook
Chapter 19, Problem 51
Using S° values from Appendix C, calculate ΔS° values for the following reactions. In each case, account for the sign of ΔS°.
(a) C2H4(g) + H2(g) → C2H6(g)
(b) N2O4(g) → 2 NO2(g)
(c) Be(OH)2(s) → BeO(s) + H2O(g)
(d) 2 CH3OH(g) + 3 O2(g) ⟶ 2 CO2(g) + 4 H2O(g)
Verified step by step guidance1
Identify the standard entropy (S°) values for each reactant and product from Appendix C. You will need the S° values for CH₃OH(g), O₂(g), CO₂(g), and H₂O(g).
Multiply the S° value of each reactant and product by their respective stoichiometric coefficients in the balanced chemical equation. For reactants: 2 S°(CH₃OH(g)) + 3 S°(O₂(g)), and for products: 2 S°(CO₂(g)) + 4 S°(H₂O(g)).
Sum up the total S° values for all reactants and all products separately. This will give you two totals: one for the reactants and one for the products.
Calculate the change in entropy (ΔS°) for the reaction by subtracting the total S° value of the reactants from the total S° value of the products: ΔS° = [2 S°(CO₂(g)) + 4 S°(H₂O(g))] - [2 S°(CH₃OH(g)) + 3 S°(O₂(g))].
Analyze the sign of ΔS°. If ΔS° is positive, it indicates an increase in disorder or randomness in the system as the reaction proceeds. If ΔS° is negative, it indicates a decrease in disorder.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Standard Entropy (S°)
Standard entropy (S°) is a measure of the randomness or disorder of a system at a standard state, typically defined at 1 bar of pressure and a specified temperature, usually 298 K. It reflects the number of accessible microstates for a given substance, with higher values indicating greater disorder. In chemical reactions, the change in entropy (ΔS°) can be calculated by considering the standard entropies of the reactants and products.
Entropy Change (ΔS°)
The change in entropy (ΔS°) for a reaction is calculated using the formula ΔS° = ΣS°(products) - ΣS°(reactants). This value indicates whether the disorder of the system increases or decreases during the reaction. A positive ΔS° suggests an increase in disorder, while a negative ΔS° indicates a decrease. Understanding the sign of ΔS° is crucial for predicting the spontaneity of a reaction.
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Gas Phase Reactions and Entropy
In gas phase reactions, the number of moles of gaseous reactants and products significantly influences the entropy change. Generally, reactions that produce more gas molecules than they consume lead to an increase in entropy (positive ΔS°), while those that consume more gas molecules result in a decrease in entropy (negative ΔS°). This concept is essential for analyzing the given reaction, where the number of gaseous reactants and products must be compared to determine the sign of ΔS°.
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