A chemical reaction involves the reactants A and B, and the product C. Use the experimental data below and the method of initial rates to determine the rate law for the reaction and the value of the rate constant. A B C Trial [A](m) [B](mol) A[A] mol At L s 1 0.025 0.025 0.03984375 2 0.025 0.050 0.31875 3 0.050 0.025 0.03984375 Complete the rate law expression and give the value of k below. • Complete the rate law expression in the left box in terms of the concentration of A, [A], and/or B, [B]. • Do not include a comma in your answer. • Simplify the rate law (do not include unnecessary exponents). . Report your value of k in the right box with two significant figures, do not include units. Provide your answer below: rate = k k = =

A chemical reaction involves the reactants A and B, and the product C. Use the experimental data below and the method of initial rates to determine the rate law for the reaction and the value of the rate constant. A B C Trial [A](m) [B](mol) A[A] mol At L s 1 0.025 0.025 0.03984375 2 0.025 0.050 0.31875 3 0.050 0.025 0.03984375 Complete the rate law expression and give the value of k below. • Complete the rate law expression in the left box in terms of the concentration of A, [A], and/or B, [B]. • Do not include a comma in your answer. • Simplify the rate law (do not include unnecessary exponents). . Report your value of k in the right box with two significant figures, do not include units. Provide your answer below: rate = k k = =

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 7ALQ

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The reaction NO(g) + O,(g) — NO,(g) + 0(g) plays a role in the formation of nitrogen dioxide in automobile engines. Suppose that a series of experiments measured the rate of this reaction at 500 K and produced the following data; [NO] (mol L ’) [OJ (mol L 1) Rate = -A[NO]/Af (mol L_1 s-1) 0.002 0.005 8.0 X 10"'7 0.002 0.010 1.6 X 10-'6 0.006 0.005 2.4 X IO-'6 Derive a rate law for the reaction and determine the value of the rate constant.
Can a reaction mechanism ever be proven correct? Can it be proven incorrect?
11.35 For the reaction 2 NO(g) + 2 H?(g) — N,(g) + 2 H,O(g) at 1100°C, the following data have been obtained: [NOJ [HJ Rate = A(N2]/At (mol L~1) (mol L_1) (mol L-1 s_1) 5.0 X 10’1 0.32 0.012 1.0 X 10~’ 0.32 0.048 1.0 X 10"2 0.64 0.096 Derive a rate law for the reaction and determine the value of the rate constant.
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.
In Chapter 3, we discussed the conversion of biomass into biofuels. One important area of research associated with biofuels is the identification and development of suitable catalysts to increase the rate at which fuels can be produced. Do a web search to find an article describing biofuel catalysts. Then, write one or two sentences describing the reactions being catalyzed, and identify the catalyst as homogeneous or heterogeneous.
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
For the reaction A + B C, explain at least two ways in which the rate law could be zero order in chemical A.
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?
Use the PhET Reactions Single collision tab of the simulation applet, enable the Energy view" by clicking the + icon. Select the first A+BCAB+C reaction (A is yellow, B is purple. and C is navy blue). Using the angled shut option, try launching the A atom with varying angles, but with more Total energy than the transition state. What happens when the A atom hits the BC molecule from different directions? Why?
Explain what is meant by the average rate of a reaction.
At low temperatures, the rate law for the reaction CO(g)+NO2(g)CO2(g)+NO(g)is as follows: rate=(constant)[ NO2 ]2. Which of the following mechanisms is consistent with the rate law? (a) CO+NO2CO2+NO(b) 2NO2N2O4(fast) N2O4+2CO2CO2+2NO(slow) (c) 2NO2NO3+NO(slow) NO3+CONO2+CO2(fast) (d) 2NO22NO+O2(slow) O2+2CO2CO2(fast)

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