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A certain reaction has the following general form: aA + bB At a particular temperature and [A], = 4.80 x 10-8 M, concentration versus time data were collected for this reaction, and a plot of 1/[A] versus time resulted in a straight line with a slope value of +2.04 x 10-2 L/mol-s. a Determine the rate law for this reaction. (Use k for the rate constant.) Rate = k[A]? Determine the integrated rate law for this reaction. 1 [A] +kt [A]o Determine the value of the rate constant for this reaction. Rate constant = 2.04x10^-2 V L · mol-.s-1 b Calculate the half-life for this reaction. Half-life = 1.02x10^4 c How much time is required for the concentration of A to decrease to 7.00 x 10-4 M? Time =

A certain reaction has the following general form: aA + bB At a particular temperature and [A], = 4.80 x 10-8 M, concentration versus time data were collected for this reaction, and a plot of 1/[A] versus time resulted in a straight line with a slope value of +2.04 x 10-2 L/mol-s. a Determine the rate law for this reaction. (Use k for the rate constant.) Rate = k[A]? Determine the integrated rate law for this reaction. 1 [A] +kt [A]o Determine the value of the rate constant for this reaction. Rate constant = 2.04x10^-2 V L · mol-.s-1 b Calculate the half-life for this reaction. Half-life = 1.02x10^4 c How much time is required for the concentration of A to decrease to 7.00 x 10-4 M? Time =

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions
Section: Chapter Questions
Problem 12PS: The reaction 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) was studied at 904 C, and the data in the table...
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A certain reaction has the following general form: aA + bB At a particular temperature and [A], = 4.80 x 10-8 M, concentration versus time data were collected for this reaction, and a plot of 1/[A] versus time resulted in a straight line with a slope value of +2.04 x 10-2 L/mol-s. a Determine the rate law for this reaction. (Use k for the rate constant.) Rate = k[A]? Determine the integrated rate law for this reaction. 1 [A] +kt [A]o Determine the value of the rate constant for this reaction. Rate constant = 2.04x10^-2 V L · mol-.s-1 b Calculate the half-life for this reaction. Half-life = 1.02x10^4 How much time is required for the concentration of A to decrease to 7.00 x 104 M? Time =
Transcribed Image Text:A certain reaction has the following general form: aA + bB At a particular temperature and [A], = 4.80 x 10-8 M, concentration versus time data were collected for this reaction, and a plot of 1/[A] versus time resulted in a straight line with a slope value of +2.04 x 10-2 L/mol-s. a Determine the rate law for this reaction. (Use k for the rate constant.) Rate = k[A]? Determine the integrated rate law for this reaction. 1 [A] +kt [A]o Determine the value of the rate constant for this reaction. Rate constant = 2.04x10^-2 V L · mol-.s-1 b Calculate the half-life for this reaction. Half-life = 1.02x10^4 How much time is required for the concentration of A to decrease to 7.00 x 104 M? Time =
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