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Consider the hypothetical reaction A+B+2C 2D+3E where the rate law is Δ[Α] At Rate == = k[A][B]² An experiment is carried out where [A] = 1.0 x 10-2 M, [B] = 3.0 M, and [Clo = 2.0 M. The reaction is started, and after 7.0 seconds, the concentration of A is 3.8 x 10-³ M. a. Calculate the value of k for this reaction. L² mol 28-¹1 b. Calculate the half-life for this experiment. k=

Consider the hypothetical reaction A+B+2C 2D+3E where the rate law is Δ[Α] At Rate == = k[A][B]² An experiment is carried out where [A] = 1.0 x 10-2 M, [B] = 3.0 M, and [Clo = 2.0 M. The reaction is started, and after 7.0 seconds, the concentration of A is 3.8 x 10-³ M. a. Calculate the value of k for this reaction. L² mol 28-¹1 b. Calculate the half-life for this experiment. k=

Chemistry by OpenStax (2015-05-04)
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 25E: Nitrogen monoxide reacts with chlorine according to the equation: 2NOCI(g)2NOCI(g) The following...
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Consider the hypothetical reaction A+B+ 2C 2D + 3E where the rate law is Δ[Α] At Rate = == = k[A][B]² An experiment is carried out where [Alo 1.0 x 10-2 M, = [Blo = 3.0 M, and [Cl = 2.0 M. The reaction is started, and after 7.0 seconds, the concentration of A is 3.8 x 10-³ M. a. Calculate the value of k for this reaction. L² mol 28-1 k= b. Calculate the half-life for this experiment. Half-life = S c. Calculate the concentration of A after 12.0 seconds. Concentration = d. Calculate the concentration of C after 12 seconds. Concentration = Submit Answer 9 more group attempts remaining Retry Entire Group M M
Transcribed Image Text:Consider the hypothetical reaction A+B+ 2C 2D + 3E where the rate law is Δ[Α] At Rate = == = k[A][B]² An experiment is carried out where [Alo 1.0 x 10-2 M, = [Blo = 3.0 M, and [Cl = 2.0 M. The reaction is started, and after 7.0 seconds, the concentration of A is 3.8 x 10-³ M. a. Calculate the value of k for this reaction. L² mol 28-1 k= b. Calculate the half-life for this experiment. Half-life = S c. Calculate the concentration of A after 12.0 seconds. Concentration = d. Calculate the concentration of C after 12 seconds. Concentration = Submit Answer 9 more group attempts remaining Retry Entire Group M M
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