Some measurements of the initial rate of a certain reaction are given in the table below.N2 H2 initial rate of reaction1.40M0.148 M0.0496 M/s1.40M 0.220M0.0737 M/s2.75 M 0.148 M0.191 M/sUse 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 3 significant digits. Also be sure your answer has the correct unit symbol.rate = k||

We have to calculate the rate constant and rate law expression for the following chemical…

Answered: Some measurements of the initial rate…

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 33E: The reaction I(aq)+OCl(aq)IO(aq)+Cl(aq) was studied, and the following data were obtained:...

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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
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
Explain what is meant by the average rate of a reaction.
Experiments were conducted to study the rate of the reaction represented by this equation.[2] 2NO(g)+2H2(g)N2(g)+2H2O(g) Initial concentrations and rates of reaction are given here. Experiment Initial Concentration [NO] (mol/L) Initial Concentration, [H2] (mol/L) Initial Rate of Formation of N2 (mol/L min) 1 0.0060 0.0010 1.8104 2 0.0060 0.0020 3.6104 3 0.0010 0.0060 0.30104 4 0.0020 0.0060 1.2104 Consider the following questions: (a) Determine the order for each of the reactants, NO and H2, from the data given and show your reasoning. (b) Write the overall rate law for the reaction. (c) Calculate the value of the rate constant, k, for the reaction. Include units. (d) For experiment 2, calculate the concentration of NO remaining when exactly one-half of the original amount of H2 had been consumed. (e) The following sequence of elementary steps is a proposed mechanism for the reaction. Step 1: NO+NON2O2 Step 2: N2O2+H2H2O+N2O Step 3: N2O+H2N2+H2O Based on the data presented, which of these is the rate determining step? Show that the mechanism is consistent with the observed rate law for the reaction and the overall stoichiometry of the reaction.
Nitrogen monoxide reacts with chlorine according to the equation: 2NOCI(g)2NOCI(g) The following initial rates of reaction have been observed for certain reactant concentrations: [NO] (moI/L1) [CI2] (mol/L) Rate (moI/L/h) 0.50 0.50 1.14 1.00 0.50 4.56 1.00 1.00 9.12 What is the rate equation that describes the rate’s dependence on the concentrations of NO and CI2? What is the rate constant? What are the orders with respect to each reactant?
The enzyme carbonic anhydrase catalyzes the transformation of carbon dioxide into hydrogen carbonate ions. This reaction was studied by H. DeVoe and G. B. Kistiakowsky (Journal of the American Chemical Society, Vol. 83, p. 274, 1961) and found to obey the Michaelis-Menten model. Use the data below at a given temperature to calculate the maximum rate of the reaction. Ratemax. See Question 45 for the graphical method to use.
The reaction I(aq)+OCl(aq)IO(aq)+Cl(aq) was studied, and the following data were obtained: [I]0(mol/L) [OCl]0(mol/L) Initial Rate (mol/L s) 0.12 0.18 7.91 102 0.060 0.18 3.95 102 0.030 0.090 9.88 103 0.24 0.090 7.91 102 a. What is the rate law? b. Calculate the value of the rate constant. c. Calculate the initial rate for an experiment where both Iand OCl are initially present at 0.15 mol/L.
The decomposition of hydrogen peroxide was studied, and the following data were obtained at a particular temperature: Time(s) [H2O2](mol/L) 0 1.00 120 1 0.91 300 1 0.78 600 1 0.59 1200 1 0.37 1800 1 0.22 2400 1 0.13 3000 1 0.082 3600 1 0.050 Assuming that Rate=[H2O2]t determine the rate law, the integrated rate law, and the value of the rate constant. Calculate [H2O2] at 4000. s after the start of the reaction.
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.
Experimental data are listed here for the reaction B: Time (s) IB] (mol/L) 0.00 0.000 10.0 0.326 20.0 0.572 30.0 0.750 40.0 0.890 Prepare a graph from these data, connect the points with a smooth line, and calculate the rate of change of [B] for each 10-s interval from 0.0 to 40.0 s. Does the rate of change decrease from one time interval to the next? Suggest a reason for this result. How is the rate of change of [AJ related to the rate of change of [B] in each time interval? Calculate the rate of change of [AJ for the time interval from 10.0 to 20.0 s. What is the instantaneous rate, A[B]/Ar, when [BI = 0.750 mol/L?
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).
Consider the general reaction aA+bBcC and the following average rate data over some time period t: At=0.0080mol/LsBt=0.0120mol/LsCt=0.0160mol/Ls Determine a set of possible coefficients to balance this general reaction.

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