The rate of a certain reaction is given by the following rate law:rate=k [NO] ² [0₂]Use this information to answer the question below.The rate of the reaction is measured to be 4.0x 103 M/s when [NO] = 1.8 M and [0₂] =0.54 M. Calculate the value of the rateconstant. Be sure your answer has the correctnumber of significant digits.k = M².S Some measurements of the initial rate of a certain reaction are given in the table below.[1¹2] initial rate of reaction3.00 × 10³ M/s5.19 × 10³ M/s1.35 × 10³ M/s2.09M 0.277 M2.09M 0.479 M0.941 M 0.277 MUse this information to write a rate law for this reaction, and calculate the value of the rate constant k.Round your value for the rate constant to 2 significant digits. Also be sure your answer has the correct unit symbol.rate - DD.DX

Answered: Image /qna-images/answer/1f94be22-5727-4126-99c6-b16eb75fa7f6.jpg

The rate of a certain reaction is given by the following rate law: rate=k[NO]¹[0₂] Use this information to answer the question below. The rate of the reaction is measured to be 4.0 X 103 M/s when [NO]= 1.8 M and [0₂] = 0.54 M. Calculate the value of the rate constant. Be sure your answer has the correct number of significant digits. k=M²².s ¹ S

The rate of a certain reaction is given by the following rate law: rate=k[NO]¹[0₂] Use this information to answer the question below. The rate of the reaction is measured to be 4.0 X 103 M/s when [NO]= 1.8 M and [0₂] = 0.54 M. Calculate the value of the rate constant. Be sure your answer has the correct number of significant digits. k=M²².s ¹ S

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 31E: The decomposition of nitrosyl chloride was studied: 2NOCl(g) 2NO(g) + Cl2(g) The following data...

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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?
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?
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
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.
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Experiments show that the reaction of nitrogen dioxide with fluorine, 2 NO2(g) + F2(g) —* 2 FNO2(g) has the rate law Rate = *[NO2][FJ The reaction is thought to occur in two steps. Step 1: NO2(g) + F,(g) —* FNO,(g) + F(g) Step 2: NO2(g) + F(g) — FNO2(g) Show that the sum of this sequence of reactions gives the balanced equation for the overall reaction. Which step is rate determining?
In Exercise 11.39, if the initial concentration of N2Oj is 0.100 .\1. how long will it take for the concentration to drop to 0.0100 times its original value? The decomposition of N2O5 in solution in carbon tetrachloride is a first-order reaction: 2N2O5—»4NO2 + O2 The rate constant at a given temperature is found to be 5.25 X 10-4 s-’. If the initial concentration of N2O5 is 0.200 M, what is its concentration after exactly 10 minutes have passed?
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?
The following statements relate to the reaction for the formation of HI: H2(g) + I2(g) 2 HI(g)Rate = k[H2][I2] Determine which of the following statements are true. If a statement is false, indicate why it is incorrect. (a) The reaction must occur in a single step. (b) This is a second-order reaction overall. (c) Raising the temperature will cause the value of k to decrease. (d) Raising the temperature lowers the activation energy for this reaction. (e) If the concentrations of both reactants are doubled, the rate will double. (f) Adding a catalyst in the reaction will cause the initial rate to increase.
Compare the functions of homogeneous and heterogeneous catalysts.
The following statements relate to the reaction for the formation of HI: H2(g) + I2(g) -* 2 HI(g) Rate = it[HJ [I2J Determine which of the following statements are true. If a statement is false, indicate why it is incorrect. The reaction must occur in a single step. This is a second-order reaction overall. Raising the temperature will cause the value of k to decrease. Raising the temperature lowers the activation energy' for this reaction. If the concentrations of both reactants are doubled, the rate will double. Adding a catalyst in the reaction will cause the initial rate to increase.