Given reaction rate data for: H2O2 + 31 + 2H* → I3 ¯ + 2H2O Trial [H2O2] M [1'] M [H'] M Rate (M/s) 1.15 x 106 2.30 x 106 2.30 x 106 1.15 x 106 0.010 0.020 0.010 0.010 0.020 1 0.00050 2 0.00050 0.010 0.010 3 0.00050 0.00100 4 0.010 Write the rate law for the reaction. O a. Rate = k[H2O2][I¯ ][H¯] O b. Rate = k[H2O2]²[I* ][H¯ ] O c. Rate = k[H2O2]²[I" ] O d. Rate = k[H2O2][I" ]?[H¯ ] O e. Rate = k[H2O2][I¯ ]
Given reaction rate data for: H2O2 + 31 + 2H* → I3 ¯ + 2H2O Trial [H2O2] M [1'] M [H'] M Rate (M/s) 1.15 x 106 2.30 x 106 2.30 x 106 1.15 x 106 0.010 0.020 0.010 0.010 0.020 1 0.00050 2 0.00050 0.010 0.010 3 0.00050 0.00100 4 0.010 Write the rate law for the reaction. O a. Rate = k[H2O2][I¯ ][H¯] O b. Rate = k[H2O2]²[I* ][H¯ ] O c. Rate = k[H2O2]²[I" ] O d. Rate = k[H2O2][I" ]?[H¯ ] O e. Rate = k[H2O2][I¯ ]
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter12: Kinetics
Section: Chapter Questions
Problem 1E: What is the difference between average rate, initial rate, and instantaneous rate?
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Question
![Given reaction rate data for: H2O2 + 31" + 2H* → I3 ¯ + 2H2O
Trial
[H2O2] M
[1'] M
[H'] M
Rate (M/s)
1.15 х 10
2.30 x 106
2.30 x 106
1.15 x 106
1
0.010
0.020
0.010
0.010
0.020
0.010
0.00050
0.00050
0.00050
0.00100
3
4
0.010
0.010
Write the rate law for the reaction.
O a. Rate = k[H2O2][I¯ ][H¯ ]
O b. Rate = k[H202]²[I¯ ][H¯ ]
O c. Rate = k[H2O2]?[I" ]
O d. Rate = k[H2O2][I¯ ]?[H¯ ]
O e. Rate = k[H2O2][I¯ ]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F84255d44-2849-4618-810f-18751c351dca%2Fb50c8ec5-1ac8-48df-bbdd-9e72377d5fd9%2Fp8g55d9_processed.png&w=3840&q=75)
Transcribed Image Text:Given reaction rate data for: H2O2 + 31" + 2H* → I3 ¯ + 2H2O
Trial
[H2O2] M
[1'] M
[H'] M
Rate (M/s)
1.15 х 10
2.30 x 106
2.30 x 106
1.15 x 106
1
0.010
0.020
0.010
0.010
0.020
0.010
0.00050
0.00050
0.00050
0.00100
3
4
0.010
0.010
Write the rate law for the reaction.
O a. Rate = k[H2O2][I¯ ][H¯ ]
O b. Rate = k[H202]²[I¯ ][H¯ ]
O c. Rate = k[H2O2]?[I" ]
O d. Rate = k[H2O2][I¯ ]?[H¯ ]
O e. Rate = k[H2O2][I¯ ]
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