McQuarrie Rock GalloglyAttempt 3presented by Macmillan LearningConsider this initial rate data at a certain temperature in the table for the reactionOH(aq)Initial ratesOCI (aq) + (aq)OI (aq) + Cl(aq)Trial[OCI ]o(M)[I]o(M)[OH-]o(M)(M/s)10.001730.00173 0.5100.00030320.00173 0.003040.5100.00053430.00265 0.00173 0.6580.00036040.001730.00304 0.9490.000287Determine the rate law.Answer Bank[OCI]²[OCI]rate k[OH™][I-]Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemistry | Publisher: University Science Books60°F4)10:31 PM5/30/2022O[OH-]²2[1-1² Answer Bankrate = k[OCI12[OC][OH][1]Determine the value of the rate constant for this reaction and the correct units.Unitsk =M-². s-1Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemistry | Publisher: University Science Books10:31 PM"60°FO5/30/2022O[OH-]2Peup

The rate law for the reaction can be written as: rate=kOCl-xI-yOH-z ......(1) Here, x is the order…

Consider this initial rate data at a certain temperature in the table for the reaction OH(aq) [I]o [OH-]o OCI (aq) + (aq) OI (aq) + Cl(aq) Trial [OCI ]o (M) (M) (M) 1 0.00173 0.00173 0.510 2 0.00173 0.00304 0.510 3 0.00265 0.00173 0.658 4 0.00173 0.00304 0.949 Determine the rate law. rate = k [OH-]² (1-1² Answer Bank [OC] [OH™] [OCI] [1] Initial rates (M/s) 0.000303 0.000534 0.000360 0.000287

Consider this initial rate data at a certain temperature in the table for the reaction OH(aq) [I]o [OH-]o OCI (aq) + (aq) OI (aq) + Cl(aq) Trial [OCI ]o (M) (M) (M) 1 0.00173 0.00173 0.510 2 0.00173 0.00304 0.510 3 0.00265 0.00173 0.658 4 0.00173 0.00304 0.949 Determine the rate law. rate = k [OH-]² (1-1² Answer Bank [OC] [OH™] [OCI] [1] Initial rates (M/s) 0.000303 0.000534 0.000360 0.000287

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section: Chapter Questions

Problem 115QRT

See similar textbooks

Similar questions

From the given data, use a graphical method to determine the order and rate constant of the following reaction: 2XY+Z Time (s) 5.0 10.0 15.0 20.0 25.0 30.0 35.0 40.0 [X](M) 0.0990 0.0497 0.0332 0.0249 0.0200 0.0166 0.0143 0.0125
Consider a reaction of the type aA products, in which the rate law is found to he rate = k[A]3 (termolecular reactions are improbable but possible). If the first half-tife of the reaction is found to he 40. s, what is the time for the second half-life? Hint: Using your calculus knowledge, derive the integrated rate law from the differential rate law for a tennolecular reaction: Rate=d[A]dt=k[A]3
For each of the following reaction diagrams, estimate the activation energy (Ea) of the reaction:
For each of the following reaction diagrams, estimate the activation energy (Ea) of the reaction:
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?
Use the data provided in a graphical method to determine the order and rate constant of the following reaction: 2PQ+W Time (s) 9.0 13.0 18.0 22.0 25.0 [P] (M) 1.077103 1.068103 1.055103 1.046103 1.039103
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.
Nitroglycerine is an extremely sensitive explosive. In a series of carefully controlled experiments, samples of the explosive were heated to 160 C and their first-order decomposition studied. Determine the average rate constants for each experiment using the following data: Initial [C3H5N3O9] (M) 4.88 3.52 2.29 1.81 5.33 4.05 2.95 1.72 t (s) 300 300 300 300 180 180 180 180 %Decomposed 52.0 52.9 53.2 53.9 34.6 35.9 36.0 35.4
A certain reaction has the form aAProducts At a particular temperature, concentration versus time data were collected. A plot of 1/ [A] versus Lime (in seconds) gave a straight line with a slope of 6.90 102. What is the differential rate law for this reaction? What is the integrated rate law for this reaction? What is the value of the rate constant for this reaction? If [A]0 for this reaction is 0.100 M, what is the first half-life (in seconds)? If the original concentration (at t = 0) is 0.100 M, what is the second half-life (in seconds)?
Go to the PhET Reactions and change to Angled shot to see the difference. (a) What happens when the angle of the collision is changed? (b) Explain how this is relevant to rate of reaction.
In the PhET Reactions under Options. (a) Leave the Initial Temperature at the default setting. Observe the reaction. Is the rate of reaction fast or slow? (b) Click Pause" and then Reset All, and then enter 15 molecules of A and 10 molecules of BC once again. Select Show Bonds" under Options. This time, increase the initial temperature until, on the graph, the total average energy line is completely above the potential energy curve. Describe what happens to the reaction.