2C4H6(g) → C8H12(g) At high temperatures, the compound C4H6 (1,3-butadiene) reacts according to the equation above. The rate of the reaction was studied at 625 K in a rigid reaction vessel. Two different trials, each shown with a different starting concentration, were carried out. The data were plotted in three different ways, as shown below. (a) For trial 1, calculate the initial pressure, in atm, in the vessel at 625 K. Assume that initially all the gas present in the vessel is C4H6. (Hint-this is a gas law problem from chemistry last year) (b) Use the data plotted in the graphs to determine the order of the reaction with respect to C4H6. (c) The initial rate of the reaction in trial 1 is 0.0010 mol/(L *s). Calculate the rate constant, k, for the reaction at 625 K.
2C4H6(g) → C8H12(g) At high temperatures, the compound C4H6 (1,3-butadiene) reacts according to the equation above. The rate of the reaction was studied at 625 K in a rigid reaction vessel. Two different trials, each shown with a different starting concentration, were carried out. The data were plotted in three different ways, as shown below. (a) For trial 1, calculate the initial pressure, in atm, in the vessel at 625 K. Assume that initially all the gas present in the vessel is C4H6. (Hint-this is a gas law problem from chemistry last year) (b) Use the data plotted in the graphs to determine the order of the reaction with respect to C4H6. (c) The initial rate of the reaction in trial 1 is 0.0010 mol/(L *s). Calculate the rate constant, k, for the reaction at 625 K.
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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2C4H6(g) → C8H12(g)
At high temperatures, the compound C4H6 (1,3-butadiene) reacts according to the equation above. The
(a) For trial 1, calculate the initial pressure, in atm, in the vessel at 625 K. Assume that initially all
the gas present in the vessel is C4H6. (Hint-this is a
(b) Use the data plotted in the graphs to determine the order of the reaction with respect to C4H6.
(c) The initial rate of the reaction in trial 1 is 0.0010 mol/(L *s). Calculate the rate constant, k, for
the reaction at 625 K.
![[C₂H] (mol/L)
0.0209
0.015
0.010
0.005-
0-
0
[C₂H₂] vs. Time
gooog
·10
20000000
10
Time (s)
1/[C₂H₂] (L/mol)
250-
200-
ooooo
0
15
150
100
500 00
0
5
20
Trial 1
▪Trial 2
1/C₂H] vs. Time
18
•
Ho
10
Time (s)
15
60
In [C₂H]
-3.5
-3.90
-4.3-
-4.7
-5.1-
-5.5-
0
20
00
Trial I
Trial 2
In [CH] vs. Time
00000
LOOOOOO00
10
Time (s)
15
20
o Trial
Trial](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F136e0cee-e194-4616-a559-a95185da047a%2Fd21642fe-d723-4f3c-823b-64321569bdb8%2Fgdx4a5r_processed.png&w=3840&q=75)
Transcribed Image Text:[C₂H] (mol/L)
0.0209
0.015
0.010
0.005-
0-
0
[C₂H₂] vs. Time
gooog
·10
20000000
10
Time (s)
1/[C₂H₂] (L/mol)
250-
200-
ooooo
0
15
150
100
500 00
0
5
20
Trial 1
▪Trial 2
1/C₂H] vs. Time
18
•
Ho
10
Time (s)
15
60
In [C₂H]
-3.5
-3.90
-4.3-
-4.7
-5.1-
-5.5-
0
20
00
Trial I
Trial 2
In [CH] vs. Time
00000
LOOOOOO00
10
Time (s)
15
20
o Trial
Trial
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