ICE tables are used for calculating changes in concentration in an equilibrium system. I represents the initial concentration, C the change in concentration between the initial value and the equilibrium value, and E the final concentration at equilibrium. The equilibrium constant, K, for the following hypothetical system is 12.0 at 373 K. A(g) + 3 B(g) = C(g) + 2 D(g) The initial concentrations of A, B, C, and D are 0.80 M, 0.40 M, 2.0 M, and 0.60 M respectively. Calculate the value of Q and compare with K to determine if the system moves to the left or the right to achieve equilibrium. Then complete the ICE table to show the changes and equilibrium concentrations using the values from the following list.
ICE tables are used for calculating changes in concentration in an equilibrium system. I represents the initial concentration, C the change in concentration between the initial value and the equilibrium value, and E the final concentration at equilibrium. The equilibrium constant, K, for the following hypothetical system is 12.0 at 373 K. A(g) + 3 B(g) = C(g) + 2 D(g) The initial concentrations of A, B, C, and D are 0.80 M, 0.40 M, 2.0 M, and 0.60 M respectively. Calculate the value of Q and compare with K to determine if the system moves to the left or the right to achieve equilibrium. Then complete the ICE table to show the changes and equilibrium concentrations using the values from the following list.
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
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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So these ICE charts are a killer for me. I seem to be understanding every it these so please show you work a little but not to much. Thank you
Transcribed Image Text:ICE tables are used for calculating changes in concentration in an equilibrium system. I represents the initial concentration,
C the change in concentration between the initial value and the equilibrium value, and E the final concentration at
equilibrium.
The equilibrium constant, K, for the following hypothetical system is 12.0 at 373 K.
A(g) + 3 B(g) = C(g) + 2 D(g)
The initial concentrations of A, B, C, and D are 0.80 M, 0.40 M, 2.0 M, and 0.60 M respectively. Calculate the value of Q and
compare with K to determine if the system moves to the left or the right to achieve equilibrium. Then complete the ICE table
to show the changes and equilibrium concentrations using the values from the following list.
![-X
+X
I
C
E
-2x
+2x
[Α]
0.80
-3x +3x 0.40-x
0.60-2x 0.60 + 2x
[B]
0.40
0.80-x
[C]
2.0
0.40 - 3x
0.40 + x
0.80 + x
0.40 + 3x
2.0-x 2.0 + X
[D]
0.60
0.60-x
0.60 + x](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F67b43319-71bb-4def-806a-245c25d89877%2Ff995f531-bca2-4ec2-8540-0c74b0e94a2f%2Foamwmge_processed.jpeg&w=3840&q=75)
Transcribed Image Text:-X
+X
I
C
E
-2x
+2x
[Α]
0.80
-3x +3x 0.40-x
0.60-2x 0.60 + 2x
[B]
0.40
0.80-x
[C]
2.0
0.40 - 3x
0.40 + x
0.80 + x
0.40 + 3x
2.0-x 2.0 + X
[D]
0.60
0.60-x
0.60 + x
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