Question

Predict the sign of the entropy change of the system for each of the following reactions: (a) $\mathrm{CO}(g)+\mathrm{H}_{2}(g) \longrightarrow C(s)+\mathrm{H}_{2} \mathrm{O}(g)$ (b) $2 \mathrm{O}_{2}(g)+\mathrm{N}_{2}(g) \longrightarrow 2 \mathrm{NO}_{2}(g)$ (c) $\mathrm{NH}_{4} \mathrm{Cl}(s) \longrightarrow \mathrm{HCl}(g)+\mathrm{NH}_{3}(g)$ (d) $2 \mathrm{C}_{2} \mathrm{H}_{4}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}(g)$

Name: Problem 41, Chapter 19: Chemistry: The Central Science in SI Units, Global Edition
Uploaded: 2021-07-22T00:27:02-08:00
Duration: 2 min 38 s
Channel: Christopher Nilsen
Description: Predict the sign of the entropy change of the system for each of the following reactions: (a) CO(g)+H2(g) ⟶C(s)+H2 O(g) (b) 2 O2(g)+N2(g) ⟶2 NO2(g) (c) NH4 Cl(s) ⟶HCl(g)+NH3(g) (d) 2 C2 H4(g)+O2(g) ⟶2 C2 H4 O(g)

   Predict the sign of the entropy change of the system for each of the following reactions:
(a) $\mathrm{CO}(g)+\mathrm{H}_{2}(g) \longrightarrow C(s)+\mathrm{H}_{2} \mathrm{O}(g)$
(b) $2 \mathrm{O}_{2}(g)+\mathrm{N}_{2}(g) \longrightarrow 2 \mathrm{NO}_{2}(g)$
(c) $\mathrm{NH}_{4} \mathrm{Cl}(s) \longrightarrow \mathrm{HCl}(g)+\mathrm{NH}_{3}(g)$
(d) $2 \mathrm{C}_{2} \mathrm{H}_{4}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}(g)$

Chemistry: The Central Science in SI Units, Global Edition

Theodore L. Brown,… 14th Edition

Chapter 19, Problem 41

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Solved by Expert Christopher Nilsen

07/22/2021

Step 1

If the number of moles of gas increases, the entropy change is positive. If the number of moles of gas decreases, the entropy change is negative. Show more…

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Predict the sign of the entropy change of the system for each of the following reactions: (a) $\mathrm{CO}(g)+\mathrm{H}_{2}(g) \longrightarrow C(s)+\mathrm{H}_{2} \mathrm{O}(g)$ (b) $2 \mathrm{O}_{2}(g)+\mathrm{N}_{2}(g) \longrightarrow 2 \mathrm{NO}_{2}(g)$ (c) $\mathrm{NH}_{4} \mathrm{Cl}(s) \longrightarrow \mathrm{HCl}(g)+\mathrm{NH}_{3}(g)$ (d) $2 \mathrm{C}_{2} \mathrm{H}_{4}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}(g)$

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Key Concepts

Entropy

Entropy is a fundamental thermodynamic quantity that measures the degree of disorder or randomness in a system. It reflects how spread out energy is among the system’s particles, and in any spontaneous process, the total entropy tends to increase in accordance with the Second Law of Thermodynamics.

Phase and Mole Count Effects

The phase of the species and the number of moles of gas present in a reaction play a critical role in determining the entropy change. Gases possess significantly higher entropy than liquids or solids due to their extensive molecular motion and randomness. Consequently, reactions that increase the total number of gas molecules typically lead to a positive entropy change, whereas reactions that decrease the number of gas molecules or convert gases into condensed phases usually result in a negative entropy change.

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