000 0[A] vs TimeIn[A] vs Time1/[A] vs TimeLeast SquaresPlotIn[A]The reactionA → Cwas performed and the concentration vs. time data below collected.3time, s 0[A], mol/L 0.7041 0.4557 0.2950 0.1909 0.1236 0.07999 0.05177 0.03351 0.02169Complete the rate law for the reaction by filling in the values for the rate constant and reaction order.1Time, s2Rate = k[A]*rate constant (without units)reaction order =45678

Answered: The reaction A → C was performed and…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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000 0
[A] vs Time
In[A] vs Time
1/[A] vs Time
Least Squares
Plot
In[A]
The reaction
A → C
was performed and the concentration vs. time data below collected.
3
time, s 0
[A], mol/L 0.7041 0.4557 0.2950 0.1909 0.1236 0.07999 0.05177 0.03351 0.02169
Complete the rate law for the reaction by filling in the values for the rate constant and reaction order.
1
Time, s
2
Rate = k[A]*
rate constant (without units)
reaction order =
4
5
6
7
8

Expert Solution

Step 1

The integrated rate law for the Zero order reaction is $[A] = - k t + [A]_{o}$ . If a plot of [A] vs time (t) is a straight line then the reaction is zero order with respect to "A".

The integrated rate law for the first order reaction is $l n [A] = - k t + l n [A]_{o}$ . If a plot of ln[A] vs time (t) is a straight line then the reaction is first order with respect to "A".

The integrated rate law for the second order reaction is $1 / [A] = k t + 1 / [A]_{o}$ . If a plot of 1/[A] vs time (t) is a straight line then the reaction is second order with respect to "A".

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