The reaction in aqueous acidic solution occurs as shown by the balanced chemicalequation below:H2O2(aq) + 31 (aq) + 2 H* (aq)13 (aq) + 2 H20(I )In the first 40.0 seconds of the reaction, the concentration of I changes from 1.000M to 0.868 M. Use the information to determine the average rate of the reactionwithin the first 40.0 seconds of the reaction.3.20x10-3 M/sO 1.10x10-3 M/sO 4.40x10-3 M/s2.20x10-3 M/s

Answered: H2O2(aq) + 31 (aq) + 2 H* (aq) 13 (aq)…

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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The reaction in aqueous acidic solution occurs as shown by the balanced chemical
equation below:
H2O2(aq) + 31 (aq) + 2 H* (aq)
13 (aq) + 2 H20(I )
In the first 40.0 seconds of the reaction, the concentration of I changes from 1.000
M to 0.868 M. Use the information to determine the average rate of the reaction
within the first 40.0 seconds of the reaction.
3.20x10-3 M/s
O 1.10x10-3 M/s
O 4.40x10-3 M/s
2.20x10-3 M/s

Expert Solution

Step 1 Fundamental Step

The average rate of a reaction over a time interval is calculated by dividing the change in concentration over that time period by the time interval. For the change in concentration of a reactant, the equation, where the brackets mean "concentration of", is

$\begin{array}{rcl} R a t e & = & - \frac{[r e a c \tan t a t t_{2}] - [r e a c \tan t a t t_{1}]}{t_{2} - t_{1}} \\ R a t e & = & - \frac{∆ [r e a c \tan t]}{∆ t} \\ o r \\ R a t e & = & \frac{∆ [p r o d u c t]}{∆ t} \end{array}$

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