(a) Express the rate of reaction with respect to each of the reactants and products.[CH;CI] = [C,]} = [CH4] = [HCI]3A[CH3CI]AtA[CI2]AtA[CCI4]AtA[HCI]AtA[CH3CI]AtA[CI,]AtA[CCI4]A[HCI]AtAt_ A[CH,CI]A[CI2]A[CCI3]1A[HCI]%3DAtAtAt3.At(b) If the instantaneous rate of the reaction with respect to HCl is 0.038 M-s1, what is the instantaneous rate of the reaction with respect to CCI4?M.s 1Use correct number of significant digits;

NOTE: You have given correct Rate of Reaction in Option (2) On the basis of that i am answering…

[CH3CI] = [C1,]3 = [CH4] = [HCI]3 A[CH3CI] At A[CI2] At A[CCI4] A[HCI] At At A[CH3CI] At A[CI2] At A[CCI4] At A(HCI) 1 A[HCI] %3D At A[CH3CI] At A[CI,] At A[CCI3] At 1 A[HCI] At b) If the instantaneous rate of the reaction with respect to HCl is 0.038 M.s1, what is the instantaneous rate of the reaction with respect to CI M.s1

[CH3CI] = [C1,]3 = [CH4] = [HCI]3 A[CH3CI] At A[CI2] At A[CCI4] A[HCI] At At A[CH3CI] At A[CI2] At A[CCI4] At A(HCI) 1 A[HCI] %3D At A[CH3CI] At A[CI,] At A[CCI3] At 1 A[HCI] At b) If the instantaneous rate of the reaction with respect to HCl is 0.038 M.s1, what is the instantaneous rate of the reaction with respect to CI M.s1

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...

See similar textbooks

Similar questions

Consider the following statements: In general, the rate of a chemical reaction increases a bit at first because it takes a while for the reaction to get warmed up. After that, however, the rate of the reaction decreases because its rate is dependent on the concentrations of the reactants, and these are decreasing. Indicate everything that is correct in these statements, and indicate everything that is incorrect. Correct the incorrect statements and explain.
The hydrolysis of the sugar sucrose to the sugars glucose and fructose, C12H22O11+H2OC6H12O6+C6H12O6 follows a first-order rate equation for the disappearance of sucrose: Rate =k[C12H22O11] (The products of the reaction, glucose and fructose, have the same molecular formulas but differ in the arrangement of the atoms in their molecules.) (a) In neutral solution, k=2.11011s1 at 27 C and 8.51011s1 at 37 C. Determine the activation energy, the frequency factor, and the rate constant for this equation at 47 C (assuming the kinetics remain consistent with the Arrhenius equation at this temperature). (b) When a solution of sucrose with an initial concentration of 0.150 M reaches equilibrium, the concentration of sucrose is 1.65107M . How long will it take the solution to reach equilibrium at 27 C in the absence of a catalyst? Because the concentration of sucrose at equilibrium is so low, assume that the reaction is irreversible. (c) Why does assuming that the reaction is irreversible simplify the calculation in pan (b)?
The acid-catalyzed iodination of acetone CH3COCH3(aq) + I2(aq) CH3COCH2I(aq) + HI(aq) is a common laboratory experiment used in general chemistry courses to teach the method of initial rates. The reaction is followed spectrophotometrically by the disappearance of the color of iodine in the solution. The following data (J. P. Birk and D. L Walters, Journal of Chemical Education, Vol. 69, p. 585, 1992) were collected at 23 C for this reaction. Determine the rate law for this reaction.
What is the difference between average rate, initial rate, and instantaneous rate?
Describe how graphical methods can be used to determine the order of a reaction and its rate constant from a series of data that includes the concentration of A at varying times.
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?
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 the past 10 years, the unsaturated hydrocarbon 1, 3-butadiene (CH2 = CH - CH = CH2) has ranked 38th among the top 50 industrial Chemicals. It is used primarily for the manufacture of synthetic rubber. An isomer exists also as cyclobutene: The isomerization of cyclobutene to butadiene is first-order and the rate constant has been measured as 2.0104s1 at 150 C in a 0.53-L ?ask. Determine the partial pressure of cyclobutene and its concentration after 30.0 minutes if an isomerization reaction is carried out at 150 C with an initial pressure of 55 torr.
Regular ?ights of supersonic aircraft in the stratosphere ale of concern because such aircraft produce nitric oxide, NO, as a byproduct in the exhaust of their engines. Nitric oxide reacts with ozone, and it has been suggested that this could contribute to depletion of the ozone layer. The reaction NO+O3NO2+O2 is first order with respect to both NO and O3 with a rate constant of 2.20107 L/mol/s. What is the instantaneous rate of disappearance of NO when [NO]=3.3106 M and [O3]=5.9107M?
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.
Three first-order reactions have the following activation energies: (a) Which reaction is the fastest? (b) Which reaction has the largest half-life? (c) Which reaction has the largest rate?
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?