Consider the following reaction: CHCl3 (g) + Cl₂ (g) → CCL (g) + HCl(g) The initial rate of the reaction is measured at several different concentrations of the reactants with the following results: [CHC13] (M) [Cl₂] (M) Initial Rate (M/s) 0.010 0.010 0.0033 0.0066 0.0093 0.026 0.020 0.020 0.040 0.010 0.020 0.040 Submit Part B ✓ Correct Fractional-order reactions are not common but are occasionally observed. T show that the rate doubles when the concentration of CHCl3 is doubled, sm respect to CHCl3. However, comparing the second and third experiments of Cl2 is doubled, the rate increases by an approximate factor of 1.5. There respect to Cl₂ is fractional. From the data, determine the rate constant (k) for the reaction. Expres your answer using two significant figures. 5 ΑΣΦ k = Previous Answers Submit Provide Feedback Request Answer P Pearson ? Re M-1/2.s-1 Copyright © 2023 Pearson Education Inc. All rights reserved. | Terms of Use | Privacy Policy | Permissi

Consider the following reaction: CHCl3 (g) + Cl₂ (g) → CCL (g) + HCl(g) The initial rate of the reaction is measured at several different concentrations of the reactants with the following results: [CHC13] (M) [Cl₂] (M) Initial Rate (M/s) 0.010 0.010 0.0033 0.0066 0.0093 0.026 0.020 0.020 0.040 0.010 0.020 0.040 Submit Part B ✓ Correct Fractional-order reactions are not common but are occasionally observed. T show that the rate doubles when the concentration of CHCl3 is doubled, sm respect to CHCl3. However, comparing the second and third experiments of Cl2 is doubled, the rate increases by an approximate factor of 1.5. There respect to Cl₂ is fractional. From the data, determine the rate constant (k) for the reaction. Expres your answer using two significant figures. 5 ΑΣΦ k = Previous Answers Submit Provide Feedback Request Answer P Pearson ? Re M-1/2.s-1 Copyright © 2023 Pearson Education Inc. All rights reserved. | Terms of Use | Privacy Policy | Permissi

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 5ALQ: Consider the following statements: In general, the rate of a chemical reaction increases a bit at...

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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.
Can a reaction mechanism ever be proven correct? Can it be proven incorrect?
Consider the following statements: In general, the rate of a chemical reaction increases a bit at first because it takes a while for the reaction to get warmed up. After that, however, the rate of the reaction decreases because its rate is dependent on the concentrations of the reactants, and these are decreasing. Indicate everything that is correct in these statements, and indicate everything that is incorrect. Correct the incorrect statements and explain.
Express the rate of the reaction 2N2O(g)2N2(g)+O2(g) in terms of (b) [ N2O ] (a) [ O2 ]
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).
Azomethane decomposes into nitrogen and ethane at high temperatures according to the following equation: (CH3)2N2(g)N2(g)+C2H6(g)The rate of the reaction is followed by monitoring the disappearance of the purple color due to iodine. The following data are obtained at a certain temperature. (a) By plotting the data, show that the reaction is first-order. (b) From the graph, determine k. (c) Using k, find the time (in hours) that it takes to decrease the concentration to 0.100 M. (d) Calculate the rate of the reaction when [ (CH3)2N2 ]=0.415M.
A friend of yours states, A balanced equation tells us how chemicals interact. Therefore, we can determine the rate law directly from the balanced equations. What do you tell your friend?
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?
Nitrogen monoxide reacts with chlorine to form nitrosyl chloride. NO(g)+12Cl2(g)NOCl(g) The figure shows the increase in nitrosyl chloride concentration under appropriate experimental conditions. The concentration of nitrosyl chloride actually starts at zero, although this fact may be difficult to see in the figure. (a) Write an expression for the rate of reaction in terms of a changing concentration. (b) Calculate the average rate of reaction between 40 and 120 seconds. (c) Calculate the instantaneous rate of reaction after 80 seconds. (d) Calculate the instantaneous rate of consumption of chlorine 60 seconds after the start of the reaction.
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Candle wax is a mixture of hydrocarbons. In the reaction of oxygen with candle w ax in Figure 11.2, the rate of consumption of oxygen decreased with time after the flask was covered, and eventually' the flame went out. From the perspective of the kinetic-molecular theory, describe what is happening in the flask. FIGURE 11.2 When a candle burns in a closed container, the flame will diminish and eventually go out. As the amount of oxygen present decreases, the rate of combustion will also decrease. Eventually, the rate of combustion is no longer sufficient to sustain the flame even though there is still some oxygen present in the vessel.