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Home Q & A Board Science-Related Homework Help Chemistry (Moderator: Laser_3)
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Whelan Whelan
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9 years ago
The reaction 4 Ag(s) + O2(g) → 2 Ag2O(s) favors Ag2O at low temperature, but it favors Ag and O2 at high temperatures. How can this be explained in terms of ΔH and ΔS?
A) ΔH is negative and ΔS is negative.
B) ΔH is negative and ΔS is positive.
C) ΔH is positive and ΔS is negative.
D) ΔH is positive and ΔS is positive.
Textbook 
Introductory Chemistry Essentials

Introductory Chemistry Essentials


Edition: 5th
Author:
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hbutler2hbutler2
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#1
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9 years ago Edited: 2 years ago, bio_man
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#2
3 years ago Edited: 2 years ago, bio_man
From the given reaction it is clear that ,

Change in entropy ,∆S is negative ( More disorderness on reactant side).

.

∆H also negative for formation of Ag2O.

.

We know ,

Gibbs energy,∆G =∆H-T∆S .

.

For spontaneous reaction ∆G should be negative.

.

∆G negative at low temperature only, because at High temperature

(-T∆S ) become high positive,and ∆G become positive.

.

Hence the reaction become non spontaneous.
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