Answer
$K_c=3.883\times10^{-5}$
Work Step by Step
$[Br_2]_0=0.086\ mol\div 1.26\ L=0.068\ M$
$[Br_2]=0.068\ M(1-3.7/100)=0.657\ M$
$[Br]=2([Br_2]_0-[Br_2])=0.00505\ M$
$K_c=[Br]^2/[Br_2]=3.883\times10^{-4}$
Chemistry and Chemical Reactivity (9th Edition)
by Kotz, John C.; Treichel, Paul M.; Townsend, John R.; Treichel, David A.
Published by
Cengage Learning
ISBN 10:
1133949649
ISBN 13:
978-1-13394-964-0
Chapter 15 Principles of Chemical Reactivity: Equilibria - Study Questions - Page 583d: 31
Update this answer!
You can help us out by revising, improving and updating this answer.
Update this answerAfter you claim an answer you’ll have 24 hours to send in a draft. An editor will review the submission and either publish your submission or provide feedback.
