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Which reaction(s) will be spontaneous at all temperatures? Question 23 options: A) 4NH3(g) + O2(g) → 2N2(g) + 6H2O(g)          ΔrH = -1267 kJmol-1  B) 2NO(g) + O­2(g) → 2NO2(g)     ΔrH = -114 kJmol-1 C) N2(g) + 2O­2(g)  → 2NO2(g)     ΔrH = 66.4 kJmol-1 D) 2CH4(g) → C2H6(g) + H2(g)     ΔrH = 64.6 kJmol-1 E) 2KClO3(s) → 2KCl(s) + 3O2(g)     ΔrH = -77.6 kJmol-1

Which reaction(s) will be spontaneous at all temperatures? Question 23 options: A) 4NH3(g) + O2(g) → 2N2(g) + 6H2O(g)          ΔrH = -1267 kJmol-1  B) 2NO(g) + O­2(g) → 2NO2(g)     ΔrH = -114 kJmol-1 C) N2(g) + 2O­2(g)  → 2NO2(g)     ΔrH = 66.4 kJmol-1 D) 2CH4(g) → C2H6(g) + H2(g)     ΔrH = 64.6 kJmol-1 E) 2KClO3(s) → 2KCl(s) + 3O2(g)     ΔrH = -77.6 kJmol-1

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter17: Spontaneity, Entropy, And Free Energy
Section: Chapter Questions
Problem 1RQ: Define the following: a. spontaneous process b. entropy c. positional probability d. system e....
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Which reaction(s) will be spontaneous at all temperatures?

Question 23 options:

A)

4NH3(g) + O2(g) → 2N2(g) + 6H2O(g)          ΔrH = -1267 kJmol-1 
B)

2NO(g) + O­2(g) → 2NO2(g)     ΔrH = -114 kJmol-1
C)

N2(g) + 2O­2(g)  → 2NO2(g)     ΔrH = 66.4 kJmol-1
D)

2CH4(g) → C2H6(g) + H2(g)     ΔrH = 64.6 kJmol-1
E)

2KClO3(s) → 2KCl(s) + 3O2(g)     ΔrH = -77.6 kJmol-1

 

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