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

step 1 Okay, starting with reaction A, we have 2H2 plus O2. It gives out 2H2O liquid. This was in gaseo

Indicate and explain the sign of ΔSuniv for each process....

Indicate and explain the sign of $\Delta S_{\text {univ }}$ for each process. a. $2 \mathrm{H}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(l)$ at $298 \mathrm{~K}$ b. the electrolysis of $\mathrm{H}_{2} \mathrm{O}(l)$ to $\mathrm{H}_{2}(g)$ and $\mathrm{O}_{2}(g)$ at $298 \mathrm{~K}$ c. the growth of an oak tree from a little acorn

Indicate and explain the sign of $\Delta S_{\text {univ }}$ for each process.
a. $2 \mathrm{H}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(l)$ at $298 \mathrm{~K}$
b. the electrolysis of $\mathrm{H}_{2} \mathrm{O}(l)$ to $\mathrm{H}_{2}(g)$ and $\mathrm{O}_{2}(g)$ at $298 \mathrm{~K}$
c. the growth of an oak tree from a little acorn

Key Concepts

Entropy

Entropy is a measure of disorder or randomness in a system. In thermodynamics, it quantifies the number of microscopic configurations that correspond to a macroscopic state. An increase in entropy typically corresponds to a system moving towards greater disorder, whereas a decrease suggests a move to a more ordered state.

Second Law of Thermodynamics

The Second Law of Thermodynamics states that the total entropy of an isolated system (or the universe) always increases in a spontaneous process. This fundamental law sets the direction of natural processes, indicating that while parts of a system may spontaneously become more ordered, this is always accompanied by a greater increase in the entropy of the surroundings.

System and Surroundings

In thermodynamic processes, it is important to distinguish between the entropy changes of the system and those of its surroundings. The overall change in the entropy of the universe (?Suniv) is the sum of the entropy change in the system and the entropy change in the surroundings. For a process to be spontaneous, the positive entropy change of the surroundings must at least compensate for any decrease in the system’s entropy.

Spontaneous versus Non-Spontaneous Processes

Spontaneous processes are characterized by a net increase in the total entropy of the universe (?Suniv > 0). In contrast, non-spontaneous processes, such as those forced by an external input of energy, typically result in a net decrease in the entropy of the universe (?Suniv < 0) when considered without that external work. This concept is a direct consequence of the Second Law of Thermodynamics and is key to understanding why some reactions occur naturally while others require additional energy input.

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