The following results were obtained for the below reaction in experiments designed for the study of the rate of the reaction. A + B=> 2CExperimentInitial concentrations mol/L [A] [B]Rate of disappearance of A(M/sec)10.0300.0302.0x10-320.0300.0604.0x10-340.0600.0304.0x10-3Determine the order of the reaction with respect to A. Determine the order of the reaction with respect to B. Calculate the value of the rate constant, k for the reaction. Include units. Write the differential rate law for this reaction. What will be the initial rate of disappearance of A, if an experiment is attempted with A and B both equal to 0.060M?Write the integrated rate law for the concentration of A.Calculate the half-life for A Calculate the concentration of A in experiment 2 after 60 seconds

Rate law of reaction is : Rate (r) = k[A]x [B]y Where x = order of reaction with respect to A y =…

Answered: The following results were obtained for…

Chemistry for Engineering Students

3rd Edition

ISBN:9781285199023

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 11.52PAE

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The following results were obtained for the below reaction in experiments designed for the study of the rate of the reaction.

A + B=> 2C

Experiment	Initial concentrations mol/L [A] [B]	Rate of disappearance of A (M/sec)
1	0.030	0.030	2.0x10^-3
2	0.030	0.060	4.0x10^-3
4	0.060	0.030	4.0x10^-3

Determine the order of the reaction with respect to A.
Determine the order of the reaction with respect to B.
Calculate the value of the rate constant, k for the reaction. Include units.
Write the differential rate law for this reaction.
What will be the initial rate of disappearance of A, if an experiment is attempted with A and B both equal to 0.060M?
Write the integrated rate law for the concentration of A.
Calculate the half-life for A
Calculate the concentration of A in experiment 2 after 60 seconds

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