An initial gas sample of NOBr decomposes according to the reaction below. The decomposition of NOBr has a Kc equal to 3.07 x 10-4 at 297 K. Predict the concentration of NO at equilibrium by constructing an ICE table, writing the equilibrium constant expression, and solving for the concentration of NO at equilibrium. Complete Parts 1-3 before submitting your answer. 2 NOBr(g) = 2 NO(g) + Br₂(g) NEXT If an initial solution of 0.20 M NOBr decomposes, fill in the ICE table with the appropriate value for each involved species. Initial (M) Change (M) Equilibrium (M) 0 -2x 1 2 NOBr(g) 0.20 -2x² 0.40 0.20-x 2 +X 0.20 + x 2 NO(g) +1² 0.40 - X 3 + +2x 0.40 + x Br₂(g) RESET +2x² 0.20-2x
An initial gas sample of NOBr decomposes according to the reaction below. The decomposition of NOBr has a Kc equal to 3.07 x 10-4 at 297 K. Predict the concentration of NO at equilibrium by constructing an ICE table, writing the equilibrium constant expression, and solving for the concentration of NO at equilibrium. Complete Parts 1-3 before submitting your answer. 2 NOBr(g) = 2 NO(g) + Br₂(g) NEXT If an initial solution of 0.20 M NOBr decomposes, fill in the ICE table with the appropriate value for each involved species. Initial (M) Change (M) Equilibrium (M) 0 -2x 1 2 NOBr(g) 0.20 -2x² 0.40 0.20-x 2 +X 0.20 + x 2 NO(g) +1² 0.40 - X 3 + +2x 0.40 + x Br₂(g) RESET +2x² 0.20-2x
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
Chapter1: Chemical Foundations
Section: Chapter Questions
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Question
![An initial gas sample of NOBr decomposes according to the reaction below. The
decomposition of NOBr has a Kc equal to 3.07 x 10-4 at 297 K. Predict the concentration
of NO at equilibrium by constructing an ICE table, writing the equilibrium constant
expression, and solving for the concentration of NO at equilibrium. Complete Parts 1-3
before submitting your answer.
2 NOBr(g) = 2 NO(g) + Br₂(g)
Initial (M)
Change (M)
Equilibrium (M)
-X
0
1
If an initial solution of 0.20 M NOBr decomposes, fill in the ICE table with the appropriate value for each
involved species.
-2x
2 NOBr(g)
0.20
-2.x²
0.40
2
0.20-x
+X
0.20 + x
2 NO(g)
+1²
3
0.40-x
+
+2r
0.40 + x
NEXT
Br₂(g)
RESET
+2x²
0.20-2x](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F19cce641-b997-49dc-afd2-8bab9dcfc62b%2F0fdc0757-6b6f-464f-8af0-13c12cf4759c%2Flmb1jab_processed.jpeg&w=3840&q=75)
Transcribed Image Text:An initial gas sample of NOBr decomposes according to the reaction below. The
decomposition of NOBr has a Kc equal to 3.07 x 10-4 at 297 K. Predict the concentration
of NO at equilibrium by constructing an ICE table, writing the equilibrium constant
expression, and solving for the concentration of NO at equilibrium. Complete Parts 1-3
before submitting your answer.
2 NOBr(g) = 2 NO(g) + Br₂(g)
Initial (M)
Change (M)
Equilibrium (M)
-X
0
1
If an initial solution of 0.20 M NOBr decomposes, fill in the ICE table with the appropriate value for each
involved species.
-2x
2 NOBr(g)
0.20
-2.x²
0.40
2
0.20-x
+X
0.20 + x
2 NO(g)
+1²
3
0.40-x
+
+2r
0.40 + x
NEXT
Br₂(g)
RESET
+2x²
0.20-2x
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