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13.9 Explain what is meant by the rate law of a reaction.

13.9 Explain what is meant by the rate law of a reaction.

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter13: Rates Of Reaction
Section: Chapter Questions
Problem 13.31QP: The reaction 2A(g)A2(g) is being run in each of the following containers. The reaction is found to...
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The Rate Law Review Questions 13.9 Explain what is meant by the rate law of a reaction. 13.10 What are the units for the rate constants of zero- order, first-order, and second-order reactions? 13.11 Consider the zero-order reaction: A – product. (a) Write the rate law for the reaction. (b) What are the units for the rate constant? (c) Plot the rate of the reaction versus [A]. 13.12 On which of the following properties does the rate constant of a reaction depend? (a) reactant concen- trations, (b) nature of reactants, (c) temperature. Problems 13.13 The rate law for the reaction NH (aq) + NO, (aq) → N2(g) + 2H,O(1)
Transcribed Image Text:The Rate Law Review Questions 13.9 Explain what is meant by the rate law of a reaction. 13.10 What are the units for the rate constants of zero- order, first-order, and second-order reactions? 13.11 Consider the zero-order reaction: A – product. (a) Write the rate law for the reaction. (b) What are the units for the rate constant? (c) Plot the rate of the reaction versus [A]. 13.12 On which of the following properties does the rate constant of a reaction depend? (a) reactant concen- trations, (b) nature of reactants, (c) temperature. Problems 13.13 The rate law for the reaction NH (aq) + NO, (aq) → N2(g) + 2H,O(1)
is given by rate = k[NH ][NO;]. At 25°C, the rate constant is 3.0 x 10IM - s. Calculate the rate of the reaction at this temperature if [NH ] = 0.26 M and [NO] = 0.080 M. 13.14 Use the data in Table 13.2 to calculate the rate of the reaction at the time when [F,] = 0.010 M and [CIO:] = 0.020 M. 13.15 Consider the reaction CARIS A +B → products From the following data obtained at a certain tem- perature, determine the order of the reaction and calculate the rate constant: [A] (M) [B] (M) Rate (M/s) 3.20 x 10" 3.20 x 10- 6.40 x 10" 1.50 1.50 1.50 2.50 3.00 1.50 13.16 Consider the reaction ARIS x + Y Z From the following data, obtained at 360 K, (a) deter- mine the order of the reaction, and (b) determine the initial rate of disappearance of X when the concentra- tion of X is 0.30 M and that of Y is 0.40 M. Initial Rate of Disappearance of X (M/s) [X] (M) [Y] (M) 0.053 0.10 0.50 0.127 0.20 0.30 1.02 0.40 0.60 0.254 0.20 0.60 0.509 0.40 0.30 13.17 Determine the overall orders of the reactions to which the following rate laws apply: (a) rate = k[NO,J°, (b) rate = k, (c) rate = k[H2][Br2l, (d) rate =
Transcribed Image Text:is given by rate = k[NH ][NO;]. At 25°C, the rate constant is 3.0 x 10IM - s. Calculate the rate of the reaction at this temperature if [NH ] = 0.26 M and [NO] = 0.080 M. 13.14 Use the data in Table 13.2 to calculate the rate of the reaction at the time when [F,] = 0.010 M and [CIO:] = 0.020 M. 13.15 Consider the reaction CARIS A +B → products From the following data obtained at a certain tem- perature, determine the order of the reaction and calculate the rate constant: [A] (M) [B] (M) Rate (M/s) 3.20 x 10" 3.20 x 10- 6.40 x 10" 1.50 1.50 1.50 2.50 3.00 1.50 13.16 Consider the reaction ARIS x + Y Z From the following data, obtained at 360 K, (a) deter- mine the order of the reaction, and (b) determine the initial rate of disappearance of X when the concentra- tion of X is 0.30 M and that of Y is 0.40 M. Initial Rate of Disappearance of X (M/s) [X] (M) [Y] (M) 0.053 0.10 0.50 0.127 0.20 0.30 1.02 0.40 0.60 0.254 0.20 0.60 0.509 0.40 0.30 13.17 Determine the overall orders of the reactions to which the following rate laws apply: (a) rate = k[NO,J°, (b) rate = k, (c) rate = k[H2][Br2l, (d) rate =
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