Consider the following proposed reaction mechanism: Step 1: F2 + 2 NO2 → NO2F + F + NO2 Step 2: F + NO2 → NO2F The first step is the slow (rate-determining) step. Answer the following questions: Question 31: The intermediates in the overall equation are: F2 NO₂F NO2 F Check Question 32: If this mechanism is correct, the rate law of the overall reaction would be rate = k₁[F2][NO2] Cannot be determined rate = k₁[[NO₂F]² rate = k₁[F2]²[NO2]² rate = = K₁[F2][NO2]² Check

Consider the following proposed reaction mechanism: Step 1: F2 + 2 NO2 → NO2F + F + NO2 Step 2: F + NO2 → NO2F The first step is the slow (rate-determining) step. Answer the following questions: Question 31: The intermediates in the overall equation are: F2 NO₂F NO2 F Check Question 32: If this mechanism is correct, the rate law of the overall reaction would be rate = k₁[F2][NO2] Cannot be determined rate = k₁[[NO₂F]² rate = k₁[F2]²[NO2]² rate = = K₁[F2][NO2]² Check

Chemistry

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Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 100AE: Consider a hypothetical reaction between A and B: A + B products Use the following initial rate...

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Consider a hypothetical reaction between A and B: A + B products Use the following initial rate data to calculate the rate constant for this reaction. [A] (mol/L) [B] (mol/L) Initial Rate (mol/L s) 0.20 1.0 3.0 0.50 1.0 11.8 2.0 2.0 189.5
A friend of yours states, A balanced equation tells us how chemicals interact. Therefore, we can determine the rate law directly from the balanced equations. What do you tell your friend?
Based on the diagram in Exercise 12.83, which of the reactions has the fastest rate? Which has the slowest rate?
11.102 Suppose that you are studying a reaction and need to determine its rate law. Explain what you would need to measure in order to accomplish this in a single experiment, and how you could use graphical methods to get from the experimental data to a complete rate law.
The reaction 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) was studied at 904 C, and the data in the table were collected. (a) Determine the order of the reaction for each reactant. (b) Write the rate equation for the reaction. (c) Calculate the rate constant for the reaction. (d) Find the rate of appearance of N2 at the instant when [NO] = 0.350 mol/L and [H] = 0.205 mol/L.
Based on the kinetic theory of matter, what would the action of a catalyst do to a reaction that is the reverse of some reaction that we say is catalyzed?
Consider the following hypothetical data collected in two studies of the reaction 2A+2BC+2D Time(s) Experiment 1 [A] (mol/L) Experiment 2 [A] (mol/L) 0 1.0 102 1.0 102 10. 8.4 103 5.0 103 20. 7.1 103 2.5 103 30. ? 1.3 103 40. 5.0 103 6.3 104 In Experiment 1, [B]0 = 10.0 M. In Experiment 2, [B]0 = 20.0 M. Rate=[A]t a. Use the concentration versus time data to determine the rate law for the reaction. b. Solve for the value of the rate constant (k) for the reaction. Include units. c. Calculate the concentration of A in Experiment 1 at t =30.s
In a kinetic study of the reaction 2NO(g)+O2(g)2NO2(g) the following data were obtained for the initial rates of disappearance of NO: Obtain the rate law. What is the value of the rate constant?
Ozone, O3, in the Earths upper atmosphere decomposes according to the equation 2 O3(g) 3 O2(g) The mechanism of the reaction is thought to proceed through an initial fast, reversible step followed by a slow, second step. Step 1: Fast, reversible O3(g) O2(g) + O(g) Step 2: Slow O3(g) + O(g) 2 O2(g) (a) Which of the steps is rate-determining? (b) Write the rate equation for the rate-determining step
Consider the decomposition reaction 2X2Y+ZThe following graph shows the change in concentration with respect to time for the reaction. What does each of the curves labeled 1, 2, and 3 represent?
Nitrogen monoxide reacts with chlorine according to the equation: 2NOCI(g)2NOCI(g) The following initial rates of reaction have been observed for certain reactant concentrations: [NO] (moI/L1) [CI2] (mol/L) Rate (moI/L/h) 0.50 0.50 1.14 1.00 0.50 4.56 1.00 1.00 9.12 What is the rate equation that describes the rate’s dependence on the concentrations of NO and CI2? What is the rate constant? What are the orders with respect to each reactant?
Given the following mechanism for a chemical reaction: H2O2+IH2O+IOH2O2+IOH2O+O2+I a Write the overall reaction. b Identify the catalyst and the reaction intermediate. c With the information given in this problem, can you write the rate law? Explain.

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