3. The reaction of butadiene gas (C,H,) withitself produces C,H2 gas as follows: 2C,Ho(g) →C,H,(g). Data from this reaction is collectedand the following graphs are produced.500-5300a. Write the rate law for this reaction.b. Explain how you would find the rate-6100constant for this reaction.3000600030006000Time (s)Time (s)

Chemical kinetics is the study of the kinetics of chemical reactions. The rate of reaction depends…

3. The reaction of butadiene gas (C,H,) with itself produces C,H, gas as follows: 2C,H,(9) → C,H,(g). Data from this reaction is collected and the following graphs are produced. 500 300 a. Write the rate law for this reaction. b. Explain how you would find the rate 100 constant for this reaction. 3000 6000 3000 6000 Time (s) Time (s)

3. The reaction of butadiene gas (C,H,) with itself produces C,H, gas as follows: 2C,H,(9) → C,H,(g). Data from this reaction is collected and the following graphs are produced. 500 300 a. Write the rate law for this reaction. b. Explain how you would find the rate 100 constant for this reaction. 3000 6000 3000 6000 Time (s) Time (s)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The rate constant for the first-order decomposition of N2O5(g) to NO2(g) and O2(g) is 7.48 × 10-3 s-1 at a given temperature. Initially, the system only contains N2O5 at an initial pressure of 0.100 atm. a. Write a balanced chemical equation for this reaction. b. Find the total pressure after 100 s of the reaction.
An elementary step is defined as a chemical collision in a reaction mechanism. A collection of different types of collisions makes up the reaction mechanism, so elementary steps provide a molecular view of the overall reaction. Write the rate law for the following reaction, which represents an elementary step in a reaction. Your rate law should not include the states of matter. $$SO2Cl2(g)SO2(g)+Cl2(g)
The rate of a certain reaction is given by the following rate law: rate =k[N,]H, ° Use this information to answer the questions below. olo What is the reaction order in N,? x10 Ar What is the reaction order in H,? What is overall reaction order? At a certain concentration of N, and H2, the initial rate of reaction is 0.090 M / s. What would the initial rate of the reaction be if the concentration of N, were doubled? Round M S your answer to 2 significant digits. The rate of the reaction is measured to be 95.0 M / s when [N2] = 0.99 M and [H2] = 1.1 M. Calculate the value of the -2 -1 k = •S rate constant. Round your answer to 2 significant digits.
A chemistry graduate student is studying the rate of this reaction: 2SO3 (g) → 2SO₂(g) + O₂(g) He fills a reaction vessel with SO3 and measures its concentration as the reaction proceeds: time (minutes) 0 10. 20. 30. [so,] 0.0500M 0.0190M 0.0117 M 0.00847 M 40. 0.00663 M Use this data to answer the following questions. Write the rate law for this reaction. Calculate the value of the rate constant k. Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k k = 0 x10 ロ・ロ X
Chemical Kinetics Tutorials 1. Consider the reaction. 2HB1(g) H2(g) + Brz(g) a. Express the rate of the reaction in terms of the change in concentration of each of the reactants and products. b. In the first 25.0 s of this reaction, the concentration of HBr drops from 0.600 M to 0.512 M. Calculate the average rate of the reaction during this time interval. 2. For the reaction 2A(g) + B(g) + 3C(g), a. Determine the expression for the rate of the reaction in terms of the change in concentration of each of the reactants and products. 3. Consider the tabulated data showing the initial rate of a reaction (A » products) at several different concentrations of A. What is the order of the reaction? Write a rate law for the reaction including the value of the rate constant, k. [A] (M) Initial Rate (Ms') 0.100 0.053 0.200 0.210 0.300 0.473 4. This reaction is first order in N2O5: N2O5(g) →NO3(g) + NO2(g) The rate constant for the reaction at a certain temperature is 0.053s. a. Calculate the rate…
Consider the reaction 2 A + B → C. What is the rate law given the following experimental data? [A], M 0.180 [B], M 0.250 0.180 0.500 0.720 0.500 A. rate = [A]²[B]² ✓B. rate = [A]¹[B]¹ C. rate = [A]²[B]¹ D. rate = [A]¹[B]² rate, M/s 1.36 x 10 2.72 x 10-3 1.09 x 10-2
36 The reaction C2H5Cl →C2H4 + HCl is first order in C2H5Cl. The rate constant is 1.60 x 10-6/s. In an investigation of the decomposition of C2H5Cl an initial concentration of 0.165 mol/L was used. What will the concentration of C2H5Cl be after 125 hours? Select one: a. 0.0803 M b. 0.0703 M c. 0.0603 M d. 0.0503M
16 The reaction C2H5Cl →C2H4 + HCl is first order in C2H5Cl. The rate constant is 1.60 x 10-6/s. In an investigation of the decomposition of C2H5Cl an initial concentration of 0.165 mol/L was used. How many hours will it take for 75% of C2H5Cl to decompose? Select one: a. 241 b. 341 h c. 541 d. 841
The rate of reaction NO2(g)+ CO(g) ----> NO (g) + CO2(g) was determined in three experiments at 225 C. The results are given in the following table: a. Determine the rate law for the reaction. Calculates the value of the rate constant at 225 C. Calculate the rate of appearance of CO2 when [NO2]=[CO]= 0.527
The reaction between hydrogen and chlorine is as follows: Cl2(g) + H2(g) → 2HCl(g) Experiments show that this reaction is first order with respect to H2 and one-half order with respect to Cl2. What is the rate law? a. Rate = k [H2]1/2 [Cl2] b. Rate = k [Cl2] [H2]2 c. Rate = k [Cl2]1/2 [H2] d. Rate = k [Cl2]2 [H2]
Consider this reaction. 2A B It obeys the rate law: rate = k [A] 2 and k = 0.188 M -1 s -1 If the initial concentration of A is 0.600 M, at what time will the concentration be 50.0% of that value? Consider this reaction. 2A B It obeys the rate law: rate = k [A] 2 and k = 0.188 M -1s -1 If the initial concentration of A is 0.600 M, at what time will the concentration be 50.0% of that value? 793 s 8.87 s 182 s 9.48 x 103 s 79.1 s 3.07 x 10-3 s 1.50 x 109 s 5.22 x 10-2 s
23. Consider the following reaction: 2 NO2(g) + O3(g) N2O5(g) + O2(g) (a) The rate law for this reaction is first order in NO2(g) and first order in O3(g). What is the rate law for this reaction? Rate = k [NO2(g)] [O3(g)] Rate = k [NO2(g)]2 [O3(g)] Rate = k [NO2(g)] [O3(g)]2 Rate = k [NO2(g)]2 [O3(g)]2 Rate = k [NO2(g)] [O3(g)]3 Rate = k [NO2(g)]4 [O3(g)] (b) If the rate constant for this reaction at a certain temperature is 62500, what is the reaction rate when [NO2(g)] = 0.530 M and [O3(g)] = 1.08 M?Rate =_____ M/s.(c) What is the reaction rate when the concentration of NO2(g) is doubled, to 1.06 M while the concentration of O3(g) is 1.08 M?Rate =____ M/s