Consider the following reaction. A(g) + B(g) → AB(g) The experimental data for this reaction is given below. Experiment Initial [A] Initial [B] Initial Rate of Consumption (M/s) 1 0.17 0.24 7.20 x 10-4 2 0.34 0.24 2.88 x 10-3 3 0.17 0.12 1.80 x 10-4 What is the rate law for this reaction? а. rate = K[A][B] b. rate = KA?IB] с. rate = KIAJ[B}? d. rate = KIA?IB}? е. rate = KIAJ?

Consider the following reaction. A(g) + B(g) → AB(g) The experimental data for this reaction is given below. Experiment Initial [A] Initial [B] Initial Rate of Consumption (M/s) 1 0.17 0.24 7.20 x 10-4 2 0.34 0.24 2.88 x 10-3 3 0.17 0.12 1.80 x 10-4 What is the rate law for this reaction? а. rate = K[A][B] b. rate = KA?IB] с. rate = KIAJ[B}? d. rate = KIA?IB}? е. rate = KIAJ?

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

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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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.
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.
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 study of the rate of dimerization of C4H6 gave the data shown in the table: 2C4H6C8H12 (a) Determine the average rate of dimerization between 0 s and 1600 s, and between 1600 s and 3200 s. (b) Estimate the instantaneous rate of dimerization at 3200 s from a graph of time versus [C4H6]. What are the units of this rate? (c) Determine the average rate of formation of C8H12 at 1600 s and the instantaneous rate of formation at 3200 s from the rates found in parts (a) and (b).
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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.