3. The reaction of CO and NO2 is second order with respect to NO₂ and zero order with respect to CO. a. Write the rate law expression. x+c = K[No₂] ² [co] rates abixoib napentin tbls b. Expressing time in units of seconds, what are the units for k? K= (an/s) / m² = M-15-1 [ K[NO₂7² OMS [0][0] How does the reaction rate change if the CO concentration is decreased by a factor of 5? KINO₂]2 <[1 No₂]² new rate - Will be decreased 25 times What is the change in the rate if the concentrations of both reactants is doubled? K(NO₂7² →ald Rall new Rate = 4 Rate old 4. Using time units of hours, what would the units for k be for a reaction that is 1/ order?

3. The reaction of CO and NO2 is second order with respect to NO₂ and zero order with respect to CO. a. Write the rate law expression. x+c = K[No₂] ² [co] rates abixoib napentin tbls b. Expressing time in units of seconds, what are the units for k? K= (an/s) / m² = M-15-1 [ K[NO₂7² OMS [0][0] How does the reaction rate change if the CO concentration is decreased by a factor of 5? KINO₂]2 <[1 No₂]² new rate - Will be decreased 25 times What is the change in the rate if the concentrations of both reactants is doubled? K(NO₂7² →ald Rall new Rate = 4 Rate old 4. Using time units of hours, what would the units for k be for a reaction that is 1/ order?

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 75E: One mechanism for the destruction of ozone in the upper atmosphere is a. Which species is a...

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Consider the zero-, first-, and second-order integrated rate laws. If you have concentration versus time data for some species in a reaction, what plots would you make to prove a reaction is either zero, first, or second order? How would the rate constant, k, be determined from such a plot? What does the y-intercept equal in each plot? When a rate law contains the concentration of two or more species, how can plots be used to determine k and the orders of the species in the rate law?
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
Explain why half-lives are not normally used to describe reactions other than first order.
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The following data have been determined for the reaction: I+OCIIO+CI 1 2 3 [I] 0.10 0.20 0.30 [OCI] 0.050 0.050 0.010 Rate(mol/L/s) 3.05104 6.20104 1.83104 Determine the rate equation and the rate constant for this reaction.
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)?
One experimental procedure that can be used to determine the rate law of a reaction is the method of initial rates. What data are gathered in the method of initial rates, and how are these data manipulated to determine k and the orders of the species in the rate law? Are the units for k. the rate constant, the same for all rate laws? Explain. If a reaction is first order in A, what happens to the rate if [A] is tripled? If the initial rate for a reaction increases by a factor of 16 when [A] is quadrupled, what is the order of n? If a reaction is third order in A and [A] is doubled, what happens to the initial rate? If a reaction is zero order, what effect does [A] have on the initial rate of a reaction?
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.
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