me umerence in the rate aws Cannot be explained by how the reaction occurs.QUESTION 15The hydrolysis of t-butyl chloride in an organic solvent occurs by the reaction(CH 3) 3CBr(g) + H 20(g) (CH 3) 3OH(g) + HBr(g).The rate law is rate = k [(CH 3) 3CB1]. How would the initial rate change if the concentration of water is doubled?O The initial rate would increase by a factor of four.%3DThe initial rate would increase by a factor of three.The initial rate would not change.O The initial rate would double.Click Save and Submit to save and submit. Click Save All Ansuwers to save all answers.MacBook AirDDF52498

For any chemical reaction, the rate of reaction is defined as the change on concentration of…

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Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 1RQ: Define reaction rate. Distinguish between the initial rate, average rate, and instantaneous rate of...

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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?
Which of the reactions in Question 62 would (a) occur fastest? (b) occur slowest? (Assume equal temperatures, equal concentrations, equal frequency factors, and the same rate law for all reactions.)
One possible mechanism for the decomposition of nitryl chloride, NO2CI, is What is the overall reaction? What rate law would be derived from this mechanism? What effect does increasing the concentration of the product NO2 have on the reaction rate?
The following kinetic data are collected for the initial rates of a reaction 2 X + Z→ products: Experiment [X ]o(M) [Z]o(M) Rate (M/s) 0.25 0.25 4.0 x 10! 0.50 0.50 3.2 x 102 0.50 0.75 7.2 x 102 (a) What is the rate law for this reaction? (b) What is the value of the rate constant with proper units? (c) What is the reaction rate when the initial concentration of X is 0.75 M and that of Z is 1.25 M? 2. 3.
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) + NO: (g) - NO(g) + O:(g) was studied at a certain tem- perature. i) In one experiment, NO, was in large excess, at a concentration of 1.0 x 1013 molecules/cm with the following data collected: Time ( latomaiem) 50 x 10 1.0x 10 20 x 19x 10 68 x 10 25x 10 30 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 NO,. De- termine the overall rate law and the value of the rate constant.
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.
Experiments show that each of the following redox reac-tions is second order overall:Reaction 1: NO₂(g)+CO(g) →NO(g)+CO₂(g) Reaction 2: NO(g)+O₃(g) →NO₂(g)+O₂(g) (a) When [NO₂] in reaction 1 is doubled, the rate quadruples.Write the rate law for this reaction.(b) When [NO] in reaction 2 is doubled, the rate doubles. Writethe rate law for this reaction.(c) In each reaction, the initial concentrations of the reactantsare equal. For each reaction, what is the ratio of the initial rateto the rate when the reaction is 50% complete?(d) In reaction 1, the initial [NO₂] is twice the initial [CO].What is the ratio of the initial rate to the rate at 50% completion?(e) In reaction 2, the initial [NO] is twice the initial [O₃]. Whatis the ratio of the initial rate to the rate at 50% completion?
The reaction O₂(g) + 2 NO(g) → 2 NO₂(g) was studied at a certain temperature with the following results: (a) What is the rate law for this reaction? O Ratek [0₂(9)] [NO(g)] O Ratek [0₂(9)]² [NO(g)] O Rate = k [0₂(9)] [NO(g)]² O Ratek [0₂(9)]² [NO(g)]² O Ratek [0₂(9)] [NO(g)]³ O Rate = k [O₂(g)]* [NO(g)] (b) What is the value of the rate constant? Experiment [0₂(9)] (M) 0.0235 0.0235 0.0470 0.0470 [NO(g)] (M) 0.0235 0.0470 0.0235 0.0470 Rate (M/S) 0.158 0.633 0.317 1.27 (c) What is the reaction rate when the concentration of O₂(g) is 0.0318 M and that of NO(g) is 0.0649 M if the temperature is the same as that used to obtain the data shown above?
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.
The reaction O₂(g) + 2 NO(g) → 2 NO₂(g) was studied at a certain temperature with the following results: (a) What is the rate law for this reaction? O Rate = k [0₂(g)] [NO(g)] O Rate = k [0₂(g)]² [NO(g)] O Rate = k [0₂(g)] [NO(g)]² O Rate = k [O₂(g)]² [NO(g)]²2 O Rate = k [O₂(g)] [NO(g)]³ O Rate = k [0₂(g)]4 [NO(g)] (b) What is the value of the rate constant? Experiment M/s 1 2 3 4 [0₂(g)] (M) 0.0231 0.0231 0.0462 0.0462 [NO(g)] (M) 0.0231 0.0462 0.0231 0.0462 Rate (M/s) 0.112 0.448 0.224 0.896 (c) What is the reaction rate when the concentration of O₂(g) is 0.0437 M and that of NO(g) is 0.0567 M if the temperature is the same as that used to obtain the data shown above?
Part A For a reaction that follows the general rate law, Rate = k[A][B]², what will happen to the rate of reaction if the concentration of A is increased by a factor of 5.00? The rate will decrease by a factor of 1/25.0. O increase by a factor of 5.00. O increase by a factor of 25.0. decrease by a factor of 1/5.00. Submit Request Answer loxt >
QUESTION 5 Consider the reaction with the rate law, Rate = k{BrO3 BrHH+j2 By what factor does the rate change if the concentration of BrO3 is tripled and that of Br" is is decreased by a factor of 3? Just put in the number as a whole number or fraction.

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