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Reaction Conc. Na2S203 Conc. HCI A Abs. A Time (s) Rate (A Abs./BA Time) 1.3686611 1.5360817 1.2267196 0.9563164 1.007568 0.300349 0.01870913 0.02870913 .30 M .15 M 1 0.10 M 1.358380874 2 0.10 M 5.114311671 .30 M .30 M 3 0.050 M 65.56796601 4 0.025 M 11.3085840 Use experimental data and the rate law to calculate a rate constant for each reaction 1, 2, 3, 4. How do the rate constants compare? Should they be the same or different? Discuss in your conclusions. Report the average value of your calculations. Be sure to include units in your rate constant. The rate law of the reaction is shown below: Rate = [NazS203]¬2

Reaction Conc. Na2S203 Conc. HCI A Abs. A Time (s) Rate (A Abs./BA Time) 1.3686611 1.5360817 1.2267196 0.9563164 1.007568 0.300349 0.01870913 0.02870913 .30 M .15 M 1 0.10 M 1.358380874 2 0.10 M 5.114311671 .30 M .30 M 3 0.050 M 65.56796601 4 0.025 M 11.3085840 Use experimental data and the rate law to calculate a rate constant for each reaction 1, 2, 3, 4. How do the rate constants compare? Should they be the same or different? Discuss in your conclusions. Report the average value of your calculations. Be sure to include units in your rate constant. The rate law of the reaction is shown below: Rate = [NazS203]¬2

Chemistry for Engineering Students
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter11: Chemical Kinetics
Section: Chapter Questions
Problem 11.49PAE: The rate of photodecomposition of the herbicide piclo- ram in aqueous systems was determined by...
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Reaction Conc. Na2S½O3 Conc. HCI A Abs. A Time (s) Rate (A Abs./ga Time) 1.007568 0.300349 0.01870913 0.02870913 1 0.10 M .30 М 1.3686611 1.358380874 0.10 M .15 M 1.5360817 5.114311671 3 0.050 M .30 M 1.2267196 65.56796601 4 0.025 M .30 M 0.9563164 11.3085840 4. Use experimental data and the rate law to calculate a rate constant for each reaction 1, 2, 3, 4. How do the rate constants compare? Should they be the same or different? Discuss in your conclusions. Report the average value of your calculations. Be sure to include units in your rate constant. The rate law of the reaction is shown below: Rate = [Na2S2O3]-2
Transcribed Image Text:Reaction Conc. Na2S½O3 Conc. HCI A Abs. A Time (s) Rate (A Abs./ga Time) 1.007568 0.300349 0.01870913 0.02870913 1 0.10 M .30 М 1.3686611 1.358380874 0.10 M .15 M 1.5360817 5.114311671 3 0.050 M .30 M 1.2267196 65.56796601 4 0.025 M .30 M 0.9563164 11.3085840 4. Use experimental data and the rate law to calculate a rate constant for each reaction 1, 2, 3, 4. How do the rate constants compare? Should they be the same or different? Discuss in your conclusions. Report the average value of your calculations. Be sure to include units in your rate constant. The rate law of the reaction is shown below: Rate = [Na2S2O3]-2
Expert Solution
Introduction

The rate of a reaction can be defined as the rate of decrease in concentration of reactants or the rate of increase in concentration of product.

The rate law can be expressed in terms of powers of concentration of reactants, and the reaction constant K.
That is 

For this simple reaction 

nA→B

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