11QThe rate of a certain reaction is given by the following rate law:te=k[H₂][¹₂]Use this information to answer the questions below.Using a rate lawWhat is the reaction order in H₂?rate=What is the reaction order in I₂?What is overall reaction order?At a certain concentration of H₂ and I2, the initial rate ofreaction is 4.0 x 103 M/s. What would the initial rate of thereaction be if the concentration of H₂ were halved? Roundyour answer to 2 significant digits.The rate of the reaction is measured to be 0.070 M/s when[H₂] = 1.3 M and [1₂] = 1.9 M. Calculate the value of the rateconstant. Round your answer to 2 significant digits.2ExplanationSWCheck3ED13$4RLLF%k =tetvG Search or type URLG04/MacBook ProY&7HUX* CO+Ⓒ2022 McGraw Hill LLC. All83C

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Using a rate law rate of a certain reaction is given by the following rate law: rate=k[H₂][¹₂] this information to answer the questions below. What is the reaction order in H₂? What is the reaction order in 1₂? What is overall reaction order? at a certain concentration of H₂ and I2, the initial rate of eaction is 4.0 x 103 M/s. What would the initial rate of the eaction be if the concentration of H₂ were halved? Round our answer to 2 significant digits. me rate of the reaction is measured to be 0.070 M/s when H2] = 1.3 M and [1₂] = 1.9 M. Calculate the value of the rate onstant. Round your answer to 2 significant digits. nation 1169 Check OCT 13 k=OM¹ (@a tv 0%

Using a rate law rate of a certain reaction is given by the following rate law: rate=k[H₂][¹₂] this information to answer the questions below. What is the reaction order in H₂? What is the reaction order in 1₂? What is overall reaction order? at a certain concentration of H₂ and I2, the initial rate of eaction is 4.0 x 103 M/s. What would the initial rate of the eaction be if the concentration of H₂ were halved? Round our answer to 2 significant digits. me rate of the reaction is measured to be 0.070 M/s when H2] = 1.3 M and [1₂] = 1.9 M. Calculate the value of the rate onstant. Round your answer to 2 significant digits. nation 1169 Check OCT 13 k=OM¹ (@a tv 0%

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 11.30PAE: The rate of the decomposition of hydrogen peroxide, H2O2, depends on the concentration of iodide ion...

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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?
Most reactions occur by a series of steps. The energy profile for a certain reaction that proceeds by a two-step mechanism is On the energy profile, indicate a. the positions of reactants and products. b. the activation energy for the overall reaction. c. E for the reaction. d. Which point on the plot represents the energy of the intermediate in the two-step reaction? e. Which step in the mechanism for this reaction is rate determining, the first or the second step? Explain.
The decomposition of many substances on the surface of a heterogeneous catalyst shows the following behavior: How do you account for the rate law changing from first order to zero order in the concentration of reactant?
Kinetics I Consider the hypothetical reaction A(g) + 2B(g) h C(g). The four containers below represent this reaction being run with different initial amounts of A and B. Assume that the volume of each container is 1.0 L. The reaction is second order with respect to A and first order with respect to B. a Based on the information presented in the problem, write the rate law for the reaction. b Which of the containers, W, X, Y, or Z, would have the greatest reaction rate? Justify your answer. c Which of the containers would have the lowest reaction rate? Explain. d If the volume of the container X were increased to 2.0 L, how would the rate of the reaction in this larger container compare to the rate of reaction run in the 1.0-L container X? (Assume that the number of A and B atoms is the same in each case.) e If the temperature in container W were increased, what impact would this probably have on the rate of reaction? Why? f If you want to double the rate of reaction in container X, what are some things that you could do to the concentration(s) of A and B? g In which container would you observe the slowest rate of formation of C? h Assuming that A and B are not in great excess, which would have the greater impact on the rate of reaction in container W: removing a unit of B or removing a unit of A? Explain. i Describe how the rate of consumption of A compares to the rate of consumption of B. If you cannot answer this question, what additional information do you need to provide an answer? j If the product C were removed from the container as it formed, what effect would this have on the rate of the reaction?
The rate of the decomposition of hydrogen peroxide, H2O2, depends on the concentration of iodide ion present. The rate of decomposition was measured at constant temperature and pressure for various concentrations of H2O2and of KI. The data appear below. Determine the order of reaction for each substance, write the rate law, and evaluate the rate constant. Rate [H2OJ [Kll (mL min-’) (mol L ’) (mol L ’) 0.090 0.15 0.033 0.178 0.30 0.033 0.184 0.15 0.066
The decomposition of iodoethane in the gas phase proceeds according to the following equation: C2H5I(g)C2H4(g)+HI(g) At 660. K, k = 7.2 104 sl; at 720. K, k = 1.7 102 sl. What is the value of the rate constant for this first-order decomposition at 325C? If the initial pressure of iodoethane is 894 torr at 245C, what is the pressure of iodoethane after three half-lives?
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?
Isomerization of CH3NC occurs slowly when CH3NC is heated. CH3NC(g) CH3CN(g) To study the rate of this reaction at 488 K, data on [CH3NC] were collected at various times. Analysis led to the following graph. (a) What is the rate law for this reaction? (b) What is the equation for the straight line in this graph? (c) Calculate the rate constant for this reaction. (d) How long does it take for half of the sample to isomerize? (e) What is the concentration of CH3NC after 1.0 104 s?
Nitrosyl bromide, NOBr, is formed from NO and Br2: 2 NO(g) + Br2(g) 2 NOBr(g) Experiments show that this reaction is second-order in NO and first-order in Br2. (a) Write the rate equation for the reaction. (b) How does the initial reaction rate change if the concentration of Br2 is changed from 0.0022 mol/L to 0.0066 mol/L? (c) What is the change in the initial rate if the concentration of NO is changed from 0.0024 mol/L to 0.0012 mol/L?
Consider the hypothetical reaction A2(g) + B2(g) 2AB(g), where the rate law is: [A2]t=k[A2][B2] The value of the rate constant at 302C is 2.45 104 L/mol s, and at 508C the rate constant is 0.891 L/mol s. What is the activation energy for this reaction? What is the value of the rate constant for this reaction at 375C?