Organic Chemistry
9th Edition
ISBN: 9781305080485
Author: John E. McMurry
Publisher: Cengage Learning
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Chapter 6.7, Problem 11P
Interpretation Introduction
Interpretation:
Among the two reactions, one with Keq=1000 and other with Keq=0.001, which is likely to be more exergonic is to be stated.
Concept introduction:
When ΔG0 is negative, the reaction is exergonic, has a favorable equilibrium constant and occurs spontaneously. When ΔG0 is positive, the reaction is endergonic, has an unfavorable equilibrium constant and cannot occur spontaneously.
To state:
Among the two reactions, one with Keq=1000 and other with Keq=0.001, which is likely to be more exergonic.
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Calculate the energy change of the following reaction:
2NO + O2→ 2NO2
ΔH:
NO = 90.0 kJ/mol
NO2= 34.0 kJ/mol
O2= 0.0 kJ/mol
a
-180 kJ
b
-112 kJ
c
35.0 kJ
d
-248 kJ
1) Which reaction is likely to be more exergonic, one with Keq = 1000 or one with Keq = 0.001?
Using the table of average bond dissociation enthalpies at 25°C, determine which of the following reactions are energetically favorable at room temperature. Assume that ▲S = 0.
Q. CH2=CH2 + CHI3 --> CH3CH2CI3
Chapter 6 Solutions
Organic Chemistry
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