Q: The diagrams above represent a chemical reaction in which red spheres represent A atoms and blue spheres represent B atoms. Based on the first image, which of the following is the correct balanced chemical equation for the reaction, and what is the sign of $$\Delta S$$ for the system?

$$\text{A}_2 + 2 \text{B} \rightarrow 2 \text{AB}$$; $$\Delta S \u003c 0$$

Question 1

The diagrams above represent a chemical reaction in which red spheres represent A atoms and blue spheres represent B atoms. Based on the first image, which of the following is the correct balanced chemical equation for the reaction, and what is the sign of $$\Delta S$$ for the system?

Accepted Answer

$$	ext{A}_2 + 2 	ext{B} ightarrow 2 	ext{AB}$$; $$\Delta S \u003c 0$$

Question 2

Refer to the second image. Which of the following statements best describes the entropy change ($$\Delta S) $$for the reaction shown?

Accepted Answer

$$\Delta S is $$negative because the number of gas molecules decreases.

Question 3

For the reaction depicted in the first image, which of the following is TRUE regarding the spontaneity and entropy change?

Accepted Answer

The reaction could be spontaneous or nonspontaneous depending on $$\Delta H$$ and $$T$$, but $$\Delta S is $$negative.

Question 4

In the context of the second image, which of the following best explains why the entropy decreases?

Accepted Answer

The reaction converts individual atoms into molecules, reducing the number of microstates.

Question 5

Given the reaction in the first image, if the process is exothermic, under what temperature conditions is the reaction most likely to be spontaneous?

Accepted Answer

At low temperatures, because $$\Delta S is $$negative and $$\Delta H is $$negative.

Entropy and Spontaneous Processes: Visualizing Molecular Changes

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