Answered: Determine

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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Question

For the reaction

Solve this using the data in the table below. For the reaction

Determine the reaction order with respect to each of the reactants. Hint: the reaction is 3rd order overall.

Determine k using the data from trial 1.

Write the rate law.

Using the rate law you just wrote, calculate the reaction rate if
the initial [ A ] = 0.046 M, the initial [ B ] = 0.10 M, and the initial [ C ] = 0.20 M. Enter the rate as a decimal number (no scientific notation, no units) with 2 significant figures.

The following data were obtained at constant temperature:

Trial	Initial (M)	Initial (M)	Initial (M)	Initial rate (M/s)
1	0.0500	0.0500	0.0100	6.25 x 10^-3
2	0.1000	0.0500	0.0100	1.25 x 10^-2
3	0.1000	0.1000	0.0100	5.00 x 10^-2
4	0.0500	0.0500	0.0200	6.25 x 10^-3

Expert Solution

Step 1

Given:

Trial	Initial (M)	Initial (M)	Initial (M)	Initial rate (M/s)
1	0.0500	0.0500	0.0100	$6.25 \times 10^{- 3}$
2	0.1000	0.0500	0.0100	$1.25 \times 10^{- 2}$
3	0.1000	0.1000	0.0100	$5.00 \times 10^{- 2}$
4	0.0500	0.0500	0.0200	$6.25 \times 10^{- 3}$

$[A] = 0.046 M [B] = 0.10 M [C] = 0.20 M$

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