Consider the following reaction: 2 HBr( g)----> H 2( g) + Br 2( g) <------ with K = 5.3 × 10 −20. a. Write the expression for the equilibrium constant for this reaction. b. Are the reactants or products favored at equilibrium? c. Would you predict ΔH to be positive or negative? d. Are the reactants or products lower in energy? e. Would you predict this reaction to be fast or slow? Explain your choice.
Consider the following reaction: 2 HBr( g)----> H 2( g) + Br 2( g) <------ with K = 5.3 × 10 −20. a. Write the expression for the equilibrium constant for this reaction. b. Are the reactants or products favored at equilibrium? c. Would you predict ΔH to be positive or negative? d. Are the reactants or products lower in energy? e. Would you predict this reaction to be fast or slow? Explain your choice.
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter18: Principles Of Chemical Reactivity: Entropy And Free Energy
Section: Chapter Questions
Problem 49PS
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Consider the following reaction: 2 HBr( g)----> H 2( g) + Br 2( g)
<------
with K = 5.3 × 10 −20.
a. Write the expression for the equilibrium constant for this
reaction.
b. Are the reactants or products favored at equilibrium?
c. Would you predict ΔH to be positive or negative?
d. Are the reactants or products lower in energy?
e. Would you predict this reaction to be fast or slow?
Explain your choice.
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