2. For the reaction A = 3C, the initial concentration of A is 1.0 M and the initial concentration of C is 0 M. After 3 minutes the concentration of A has fallen to 0.7 M and does not change any further. a. On the plot below, label the axes. Then use a solid line to plot [A] vs time for 10.0 minutes. 0.9 0.8 0.7 0.6 0.5 0.4 0.3 0.2 0.1 2 3 4 5 6 10 b. On the same set of axes, use a dashed line to show how the [C] changes with time for 10.0 minutes. c. Write an expression for the equilibrium constant in terms of [A] and [C] (do not include actual concentrations). d. Using your answer to part c, calculate the value for K. Show all of your work. e. Another flask contains 1.2 M A and 0.5 M C. Is the reaction at equilibrium? If not, what direction will this reaction shift? Explain why the reaction will shift in this direction.
2. For the reaction A = 3C, the initial concentration of A is 1.0 M and the initial concentration of C is 0 M. After 3 minutes the concentration of A has fallen to 0.7 M and does not change any further. a. On the plot below, label the axes. Then use a solid line to plot [A] vs time for 10.0 minutes. 0.9 0.8 0.7 0.6 0.5 0.4 0.3 0.2 0.1 2 3 4 5 6 10 b. On the same set of axes, use a dashed line to show how the [C] changes with time for 10.0 minutes. c. Write an expression for the equilibrium constant in terms of [A] and [C] (do not include actual concentrations). d. Using your answer to part c, calculate the value for K. Show all of your work. e. Another flask contains 1.2 M A and 0.5 M C. Is the reaction at equilibrium? If not, what direction will this reaction shift? Explain why the reaction will shift in this direction.
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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![2. For the reaction A = 3C, the initial concentration of A is 1.0 M and the initial
concentration of C is 0 M. After 3 minutes the concentration of A has fallen to 0.7 M and
does not change any further.
a. On the plot below, label the axes. Then use a solid line to plot [A] vs time for 10.0
minutes.
0.9
0.8
0.7
0.6
0.5
0.4
0.3
0.2
0.1
2
3
4
5
6
10
b. On the same set of axes, use a dashed line to show how the [C] changes with time
for 10.0 minutes.
c. Write an expression for the equilibrium constant in terms of [A] and [C] (do not
include actual concentrations).
d. Using your answer to part c, calculate the value for K. Show all of your work.
e. Another flask contains 1.2 M A and 0.5 M C. Is the reaction at equilibrium? If not,
what direction will this reaction shift? Explain why the reaction will shift in this
direction.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4cc036c0-875d-4904-b3a0-efe208cef67a%2F60368876-80a6-45a3-80ca-2c7330e33208%2F6cbjevc.png&w=3840&q=75)
Transcribed Image Text:2. For the reaction A = 3C, the initial concentration of A is 1.0 M and the initial
concentration of C is 0 M. After 3 minutes the concentration of A has fallen to 0.7 M and
does not change any further.
a. On the plot below, label the axes. Then use a solid line to plot [A] vs time for 10.0
minutes.
0.9
0.8
0.7
0.6
0.5
0.4
0.3
0.2
0.1
2
3
4
5
6
10
b. On the same set of axes, use a dashed line to show how the [C] changes with time
for 10.0 minutes.
c. Write an expression for the equilibrium constant in terms of [A] and [C] (do not
include actual concentrations).
d. Using your answer to part c, calculate the value for K. Show all of your work.
e. Another flask contains 1.2 M A and 0.5 M C. Is the reaction at equilibrium? If not,
what direction will this reaction shift? Explain why the reaction will shift in this
direction.
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