Given the following data for the conversion of reactants (R) into products (P) over time: R→ P What is the average rate of disappearance of R over the time interval from 20 seconds to 80 seconds? Time (s) [R] 0 0.700 20 0.680 40 0.665 60 0.652 80 0.641 A) 4.47 x 101 M/s B) 5.58 x 103 M/s C) 4.71 x 101 M/s D) 6.50 x 10 4 M/s Determine the rate law for the following reaction by using the initial rates below. 2 A+B Products A) r = k [A][B] C) r = k [A][B]2 [A] [B] Rate (mol L-15-1) 0.10 0.10 1.25 x 10-7 0.10 0.20 5.00 x 10-7 0.20 0.20 1.00 x 10-6 B) r = k [A] [B]2 D) r = k [A][B] E) N/A N2O5 decomposes as follows via first order kinetics: 2 N2O54 NO2 + O2 r = k[N2O5] This reaction has a rate constant, k, of 0.76 s¹. If the initial concentration of N2Os is 10.9 M, what is the concentration of N2Os after 9.6 s? A) 8.7 x 103 M B) 3.6 x 103 M
Given the following data for the conversion of reactants (R) into products (P) over time: R→ P What is the average rate of disappearance of R over the time interval from 20 seconds to 80 seconds? Time (s) [R] 0 0.700 20 0.680 40 0.665 60 0.652 80 0.641 A) 4.47 x 101 M/s B) 5.58 x 103 M/s C) 4.71 x 101 M/s D) 6.50 x 10 4 M/s Determine the rate law for the following reaction by using the initial rates below. 2 A+B Products A) r = k [A][B] C) r = k [A][B]2 [A] [B] Rate (mol L-15-1) 0.10 0.10 1.25 x 10-7 0.10 0.20 5.00 x 10-7 0.20 0.20 1.00 x 10-6 B) r = k [A] [B]2 D) r = k [A][B] E) N/A N2O5 decomposes as follows via first order kinetics: 2 N2O54 NO2 + O2 r = k[N2O5] This reaction has a rate constant, k, of 0.76 s¹. If the initial concentration of N2Os is 10.9 M, what is the concentration of N2Os after 9.6 s? A) 8.7 x 103 M B) 3.6 x 103 M
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Chapter1: Chemical Foundations
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![Given the following data for the conversion of reactants (R) into products (P) over time:
R→ P
What is the average rate of disappearance of R over the time interval from 20 seconds to 80 seconds?
Time (s)
[R]
0
0.700
20
0.680
40
0.665
60
0.652
80
0.641
A) 4.47 x 101 M/s
B) 5.58 x 103 M/s
C) 4.71 x 101 M/s
D) 6.50 x 10 4 M/s](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3cff6d5e-6d7b-4ef6-9838-a544f8e2903b%2F741382a2-a126-4948-b629-76dd497c1daf%2Fnwo1qi_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Given the following data for the conversion of reactants (R) into products (P) over time:
R→ P
What is the average rate of disappearance of R over the time interval from 20 seconds to 80 seconds?
Time (s)
[R]
0
0.700
20
0.680
40
0.665
60
0.652
80
0.641
A) 4.47 x 101 M/s
B) 5.58 x 103 M/s
C) 4.71 x 101 M/s
D) 6.50 x 10 4 M/s
![Determine the rate law for the following reaction by using the initial rates below.
2 A+B
Products
A) r = k [A][B]
C) r = k [A][B]2
[A]
[B]
Rate (mol L-15-1)
0.10
0.10
1.25 x 10-7
0.10
0.20
5.00 x 10-7
0.20
0.20
1.00 x 10-6
B) r = k [A] [B]2
D) r = k [A][B]
E) N/A
N2O5 decomposes as follows via first order kinetics:
2 N2O54 NO2 + O2
r = k[N2O5]
This reaction has a rate constant, k, of 0.76 s¹. If the initial concentration of N2Os is 10.9 M, what is the
concentration of N2Os after 9.6 s?
A) 8.7 x 103 M
B) 3.6 x 103 M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3cff6d5e-6d7b-4ef6-9838-a544f8e2903b%2F741382a2-a126-4948-b629-76dd497c1daf%2Fsm046n_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Determine the rate law for the following reaction by using the initial rates below.
2 A+B
Products
A) r = k [A][B]
C) r = k [A][B]2
[A]
[B]
Rate (mol L-15-1)
0.10
0.10
1.25 x 10-7
0.10
0.20
5.00 x 10-7
0.20
0.20
1.00 x 10-6
B) r = k [A] [B]2
D) r = k [A][B]
E) N/A
N2O5 decomposes as follows via first order kinetics:
2 N2O54 NO2 + O2
r = k[N2O5]
This reaction has a rate constant, k, of 0.76 s¹. If the initial concentration of N2Os is 10.9 M, what is the
concentration of N2Os after 9.6 s?
A) 8.7 x 103 M
B) 3.6 x 103 M
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