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

Verified step by step guidance

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.
2. 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).
3. Step 3: Consider the change in entropy of the system (ΔS_sys). 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 (ΔS_sys is negative).
4. Step 4: Consider the change in entropy of the surroundings (ΔS_surr). 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 (ΔS_surr is positive).
5. Step 5: Calculate the total change in entropy (ΔS_univ = ΔS_sys + ΔS_surr). 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 (ΔS_univ is positive), and the process is spontaneous. If not, the total entropy of the universe decreases (ΔS_univ is negative), and the process is non-spontaneous. In this case, you would need to calculate the specific values of ΔS_sys and ΔS_surr to determine the sign of ΔS_univ.

Key Concepts

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.

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.

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.