13. The kinetics of the oxidation of ethanol (C2H5OH) with dichromate (Cr2O72-) in acidic medium(H+) was studied. The table below summarizes the initial rates in four separate reactions wheredifferent initial concentrations of the reactants were used. What is the rate law for this reaction?(5 points)Cr₂0 + 3 C2H5OH + 8H+ → 2 Cr3+ + 3 CH3CHO + 7 H₂O->>>[Cr₂0]/M[C2H5OH]/M[H+]/M(rate), /Ms-10.2730.4040.3753.260.8190.4040.3759.770.2730.8080.37513.00.2730.4040.7506.52a) rate = = k[C₂H5OH][Cr2O7²¯][H+]b) rate = k[C₂H5OH]2[Cr₂O,²¯][H+]c) rate = k[C₂H5OH][Cr₂07²-]² [H+]d) rate = k[C₂H5OH]² [Cr₂O,²-]e) rate = = k [Cr₂07²¯]² [H+]²

Step 1: Step 2: Step 3: Step 4:

Answered: 13. The kinetics of the oxidation of…

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 3RQ: One experimental procedure that can be used to determine the rate law of a reaction is the method of...

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Define stability from both a kinetic and thermodynamic perspective. Give examples to show the differences in these concepts.
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The plot below shows the number of collisions with a particular energy for two different temperatures. a. Which is greater, T2 or T1? How can you tell? b. What does this plot tell us about the temperature of the rate of a chemical reaction? Explain your answer.
11.64 HBr is oxidized in the following reaction: 4 HBr(g) + O2(g) —• 2 H2O(g) + 2 Br,(g) A proposed mechanism is HBr + O2 -* HOOBr (slow) HOOBr + HBr — 2 HOBr (fast) HOBr + HBr — H2O + Bn (fast) Show that this mechanism can account for the correct stoichiometry. Identify all intermediates in this mechanism. What is the molecularity of each elementary’ step? Write the rate expression for each elementary' step. Identify the rate-determining step.
The label on a bottle of 3% (by volume) hydrogen peroxide, H2O2, purchased at a grocery store, states that the solution should be stored in a cool, dark place. H2O2decomposes slowly over time, and the rate of decomposition increases with an increase in temperature and in the presence of light. However, the rate of decomposition increases dramatically if a small amount of powdered MnO- is added to the solution. The decomposition products are H2O and O2. MnO2 is not consumed in the reaction. Write the equation for the decomposition of H2O2. What role does MnO2 play? In the chemistry lab, a student substituted a chunk of MnO2 for the powdered compound. The reaction rate was not appreciably increased. WTiat is one possible explanation for this observation? Is MnO2 part of the stoichiometry of the decomposition of H2O2?
A drug decomposes in the blood by a first-order process. A pill containing 0.500 g of the active ingredient reaches its maximum concentration of 2.5 mg/ 100 mL of blood. If the half-life of the active ingredient is 75 min, what is its concentration in the blood 2.0 h after the maximum concentration has been reached?
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Distinguish between the differential rate law and the integrated rate law. Which of these is often called just the rate law? What is k in a rate law, and what are orders in a rate law? Explain.

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