Consider the hypothetical reaction A+B+ 2C 2D + 3E where the rate law is Rate = - Δ[Α] At = k[A][B]² -2 An experiment is carried out where [A] = 1.0 × 10-² M, [B]₁ = 3.0 M, and [C] = 2.0 M. The reaction is started, and after 8.0 seconds, the concentration of A is 3.8 x 10 M. -3 a. Calculate the value of k for this reaction. L² mol 2S-1 k = 1.21 b. Calculate the half-life for this experiment. Half-life = 5.7 S c. Calculate the concentration of A after 11.0 seconds. Concentration = 2.6x10^-3 M d. Calculate the concentration of C after 11 seconds. Concentration = 2.0 M
Consider the hypothetical reaction A+B+ 2C 2D + 3E where the rate law is Rate = - Δ[Α] At = k[A][B]² -2 An experiment is carried out where [A] = 1.0 × 10-² M, [B]₁ = 3.0 M, and [C] = 2.0 M. The reaction is started, and after 8.0 seconds, the concentration of A is 3.8 x 10 M. -3 a. Calculate the value of k for this reaction. L² mol 2S-1 k = 1.21 b. Calculate the half-life for this experiment. Half-life = 5.7 S c. Calculate the concentration of A after 11.0 seconds. Concentration = 2.6x10^-3 M d. Calculate the concentration of C after 11 seconds. Concentration = 2.0 M
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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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![Consider the hypothetical reaction
A + B + 2C
2D + 3E
where the rate law is
Rate
=
Δ[Α]
At
= k[A][B]²
An experiment is carried out where [A]o
seconds, the concentration of A is 3.8 x 10
Submit Answer
-2
1.0 × 10-² M, [B] = 3.0 M, and [C] = 2.0 M. The reaction is started, and after 8.0
-3
M.
=
a. Calculate the value of k for this reaction.
-2
L² mol s
k = 1.21
b. Calculate the half-life for this experiment.
Half-life = 5.7 S
c. Calculate the concentration of A after 11.0 seconds.
Concentration = 2.6x10^-3
M
d. Calculate the concentration of C after 11 seconds.
Concentration = 2.0 M
An error has been detected in your answer. Check for typos,
miscalculations etc. before submitting your answer.
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Transcribed Image Text:Consider the hypothetical reaction
A + B + 2C
2D + 3E
where the rate law is
Rate
=
Δ[Α]
At
= k[A][B]²
An experiment is carried out where [A]o
seconds, the concentration of A is 3.8 x 10
Submit Answer
-2
1.0 × 10-² M, [B] = 3.0 M, and [C] = 2.0 M. The reaction is started, and after 8.0
-3
M.
=
a. Calculate the value of k for this reaction.
-2
L² mol s
k = 1.21
b. Calculate the half-life for this experiment.
Half-life = 5.7 S
c. Calculate the concentration of A after 11.0 seconds.
Concentration = 2.6x10^-3
M
d. Calculate the concentration of C after 11 seconds.
Concentration = 2.0 M
An error has been detected in your answer. Check for typos,
miscalculations etc. before submitting your answer.
Retry Entire Group
-1
2 more group attempts remaining
Previous
Next
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