The reaction below gave the following curve regarding rate of reaction: Cr(CO)6 + PPh3 Cr(CO)s(PPh3) + CO [PPH3), mM a) Provide a classification (in terms of the mechanism) for this reaction. Justify your answer- be sure to account for the data provided as part of your answer. b) Provide a simplified rate law for the reaction above. Rate, M/s

The reaction below gave the following curve regarding rate of reaction: Cr(CO)6 + PPh3 Cr(CO)s(PPh3) + CO [PPH3), mM a) Provide a classification (in terms of the mechanism) for this reaction. Justify your answer- be sure to account for the data provided as part of your answer. b) Provide a simplified rate law for the reaction above. Rate, M/s

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 107QRT

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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?
Question 1 (a) Distinguish between the differential rate law and the integrated rate law. Which of these is often called just the "rate law"? What is half-life of first order reaction? (b) The rate of the reaction; O(g) +NO2 (g)→NO(g) + O2(g) was studied at a certain tem- Qu perature.
(a) Select all of the correct statements about reaction rates from the choices below. The lower the rate of a reaction the longer it takes to reach completion.Reactions involving very unstable combinations of chemicals have large rate constants.Concentrations of homogeneous catalysts have no effect on reaction rates.Reaction rate constants are independent of temperature.The slowest step in a reaction is called the rate-determining step.A balanced chemical reaction is necessary to relate the rate of reaction to the concentration of a reactant.Slow reactions can be speeded up by raising the temperature.
Consider the following reaction: (a) The rate law for this reaction is first order in NO₂(g) and first order in O3(g). What is the rate law for this reaction? O Rate = k [NO₂(g)] [03(9)] Rate = k [NO₂(g)]² [03(9)] O Rate = k [NO₂(g)] [03(9)]² O Rate = k [NO₂(g)]² [03(g)]² Rate = k [NO₂(g)] [03(g)]³ Rate = k [NO₂(g)]4 [03(9)] (b) If the rate constant for this reaction at a certain temperature is 73200, what is the reaction rate when [NO₂(g)] = 0.973 M and [O3(9)] = 1.42 M? Rate = 2 NO₂(g) + 03(g) → N₂05(9) + O₂(g) M/s. Rate = (c) What is the reaction rate when the concentration of NO₂(g) is doubled, to 1.95 M while the concentration of O3(g) is 1.42 M? M/s
Determine whether the following statements are true or false, and explain your answer in one sentence. a) The rate law for an overall reaction 2A (g) -> B (g) is: Rate = k[A]^2 b) The rate law for an elementary step 2A (g) -> B (g) is: Rate = k[A]^2 c) The rate of an overal reaction is the rate of the slowest elementary step within its mechanism.
1a.) From experiment the rate law, rate = k[NO2]2, was determined for the following reaction. NO2(g) + CO(g) à NO(g) + CO2(g)Propose a mechanism. What are the intermediates? What is the molecularity of each step? 1b.) Calculate the rate constant (k) at 318 K for the following reaction (Given Ea = 52.9 kJ/mol): Mn(CO)5(CH3CN)+ + NC5H5 à Mn(CO)5(NC5H5)+ + CH3CN k min-1 T(K) 0.0409 298 0.0818 308
(a) Select all of the correct statements about reaction rates from the choices below. The lower the rate of a reaction the longer it takes to reach completion. As a reaction progresses its rate goes up. As a reaction progresses its rate goes down. Reactions involving very unstable combinations of chemicals have small rate constants. Reaction rates increase as reactant concentrations decrease. Reaction rates always increase as masses of solid reactants increase. A balanced chemical reaction is necessary to relate the rate of disappearance of a reactant to the rate of appearance of a product.
The rate of the following reaction in aqueous solution is monitored by measuring the number of moles of Hg2Cl that precipitate per liter per minute. The data obtained are listed in the table. Determine the (a) rate law and (b) rate constant (use the data for Experiment 3) 2 HgCI₂(aq) + C₂O₄-(aq) -> 2CI-(aq) + 2CO₂(g) + Hg₂Cl₂(s) Experiment 1 2 3 [H gC12](M) 0.204 0.204 0.408 [C204](M) 0.091 0.180 0.180 Initial Rate (M/s) 1.1 x10^-4 2.2x10^-4 4.4x10^-4
3. (а) (i) Given a set of data for reactant concentration versus time, outline how you would determine whether the reaction exhibited first order or second order kinetics.
Question 1 (a) Distinguish between the differential rate law and the integrated rate law. Which of these is often called just the "rate law"? What is half-life of first order reaction? (b) The rate of the reaction; O(g) + NO2 (g) → NO(g) + O2(g) was studied at a certain tem- perature. 1) In one experiment, NO2 was in large excess, at a concentration of 1.0 x 1013 molecules/cm3 with the following data collected: Time (s) (atoms/cm) 5.0 x 10 1.0x 10- 1.9 X 10 2.0 x 10- 6.8 x 10 3.0 x 10- 2.5 x 10 What is the order of the reaction with respect to oxygen atoms? ii). The reaction is known to be first order with respect to NO2. De- termine the overall rate law and the value of the rate constant.
Consider the following reaction: (a) The rate law for this reaction is first order in HBr(g) and first order in O₂(g). What is the rate law for this reaction? Rate = k [HBr(g)] [O₂(g)] O Rate = k [HBr(g)]² [O₂(g)] O Rate = k [HBr(g)] [O₂(g)]² O Rate = k [HBr(g)]² [0₂(g)]² O Rate = k [HBr(g)] [O₂(g)]³ O Rate = k [HBr(g)]4 [0₂(g)] (b) If the rate constant for this reaction at a certain temperature is 11500, what is the reaction rate when [HBr(g)] = 0.00379 M and [O₂(g)] = 0.00876 M? Rate = 4 HBr(g) + O₂(g) → 2 H₂O(g) + 2 Br₂(g) M/s. Rate = (c) What is the reaction rate when the concentration of HBr(g) is doubled, to 0.00758 M while the concentration of O₂(g) is 0.00876 M? M/S
The addition of NO accelerates the decomposition ofN2O, possibly by the following mechanism:NO(g) + N2O(g)--->N2(g) + NO2(g)2 NO2(g)--->2 NO(g) + O2(g)(a) What is the chemical equation for the overall reaction?Show how the two steps can be added to give theoverall equation. (b) Is NO serving as a catalyst or an intermediatein this reaction? (c) If experiments show thatduring the decomposition of N2O, NO2 does not accumulatein measurable quantities, does this rule out the proposedmechanism?