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Ch.19 - Free Energy & Thermodynamics
Tro - Chemistry: A Molecular Approach 5th Edition
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371Not the one you use?Change textbook
All textbooksTro 5th EditionCh.19 - Free Energy & ThermodynamicsProblem 99a
Chapter 19, Problem 99a

Indicate and explain the sign of ΔSuniv for each process. a. 2 H2(g) + O2(g) → 2 H2O (l) at 298 K.

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1
Step 1: Understand the concept of entropy (ΔS). Entropy is a measure of the randomness or disorder of a system. The second law of thermodynamics states that the total entropy of an isolated system can never decrease over time, and is constant if and only if all processes are reversible. Isolated systems spontaneously evolve towards thermodynamic equilibrium, the state with maximum entropy.
Step 2: Identify the state of the reactants and products. In this reaction, gaseous reactants (2 H2 and O2) are converted into a liquid product (2 H2O).
Step 3: Consider the change in entropy of the system (ΔSsys). The conversion of gas molecules to liquid molecules results in a decrease in randomness, as molecules in a liquid are more ordered than in a gas. Therefore, the entropy of the system decreases (ΔSsys is negative).
Step 4: Consider the change in entropy of the surroundings (ΔSsurr). The reaction is exothermic, meaning it releases heat into the surroundings. This increases the randomness of the surroundings, so the entropy of the surroundings increases (ΔSsurr is positive).
Step 5: Calculate the total change in entropy (ΔSuniv = ΔSsys + ΔSsurr). If the increase in entropy of the surroundings is greater than the decrease in entropy of the system, the total entropy of the universe increases (ΔSuniv is positive), and the process is spontaneous. If not, the total entropy of the universe decreases (ΔSuniv is negative), and the process is non-spontaneous. In this case, you would need to calculate the specific values of ΔSsys and ΔSsurr to determine the sign of ΔSuniv.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Entropy (ΔS)

Entropy is a measure of the disorder or randomness in a system. In thermodynamics, a positive change in entropy (ΔS > 0) indicates an increase in disorder, while a negative change (ΔS < 0) signifies a decrease in disorder. Understanding how entropy changes during a chemical reaction is crucial for predicting the spontaneity of the process.
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Second Law of Thermodynamics

The Second Law of Thermodynamics states that the total entropy of an isolated system can never decrease over time. It implies that natural processes tend to move towards a state of maximum disorder or entropy. This law is fundamental in determining the sign of the change in the universe's entropy (ΔS_univ) during a reaction, as it combines the entropy changes of both the system and its surroundings.
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Gibbs Free Energy (ΔG)

Gibbs Free Energy is a thermodynamic potential that helps predict the direction of chemical reactions and phase changes. It is defined as ΔG = ΔH - TΔS, where ΔH is the change in enthalpy, T is the temperature in Kelvin, and ΔS is the change in entropy. A negative ΔG indicates a spontaneous process, which is closely related to the signs of ΔS and ΔH, making it essential for analyzing the reaction's feasibility.
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Related Practice
Textbook Question

A metal salt with the formula MCl2 crystallizes from water to form a solid with the composition MCl2 • 6 H2O. The equilibrium vapor pressure of water above this solid at 298 K is 18.3 mmHg. What is the value of ΔG for the reaction MCl2 • 6 H2O(s) ⇌ MCl2(s) + 6 H2O(g) when the pressure of water vapor is 18.3 mmHg? When the pressure of water vapor is 760 mmHg?

Textbook Question

The values of ΔG°f for the hydrogen halides become less negative with increasing atomic number. The ΔG°f of HI is slightly positive. However, the trend in ΔS°f is to become more positive with increasing atomic number. Explain.

Textbook Question

The solubility of AgCl(s) in water at 25 °C is 1.33⨉10-5 mol/L and its ΔH° of solution is 65.7 kJ/mol. What is its solubility at 50.0 °C?