The questions below refer to the following information: The rate constant k for the reaction shown below is 2.6 x 100 L/mol. s when the reaction proceeds at 300.0 K. The activation energy is 98000 J/mol. (The universal gas constant, R, is 8.314 J/mol-K) 2NOCI → 2NQ + Cl₂ If the temperature changed to 350 K, the rate constant k would change. The ratio of k at 350 K to k at 300.0 K is closest to what whole number? O a. 271 O b. 274 O c. 273 O d.275 O e. 272 A Moving to another question will save this response. Co Ï O hp P IDEI <<< Question 21 of 42 ^ 1 71

The questions below refer to the following information: The rate constant k for the reaction shown below is 2.6 x 100 L/mol. s when the reaction proceeds at 300.0 K. The activation energy is 98000 J/mol. (The universal gas constant, R, is 8.314 J/mol-K) 2NOCI → 2NQ + Cl₂ If the temperature changed to 350 K, the rate constant k would change. The ratio of k at 350 K to k at 300.0 K is closest to what whole number? O a. 271 O b. 274 O c. 273 O d.275 O e. 272 A Moving to another question will save this response. Co Ï O hp P IDEI <<< Question 21 of 42 ^ 1 71

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter11: Rate Of Reaction

Section: Chapter Questions

Problem 67QAP: For the reaction 2N2O(g)2N2(g)+O2(g) the rate constant is 0.066 L/mol min at 565C and 22.8 L/mol min...

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For the reaction 2N2O(g)2N2(g)+O2(g) the rate constant is 0.066 L/mol min at 565C and 22.8 L/mol min at 728C. (a) What is the activation energy of the reaction? (b) What is k at 485C? (c) At what temperature is k, the rate constant, equal to 11.6 L/mol min?
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.
Based on the diagrams in Exercise 12.83, which of the reactions has the fastest rate? Which has the slowest rate?
Rank the following in order of increasing reaction rate. (a) Dynamite exploding (b) Iron rusting (c) Paper burning
For the decomposition of one mole of nitrosyl chloride, H = 38 kJ. NOCl(g)NO(g)+12Cl2(g) The activation energy for this reaction is 100 kJ. a Is this reaction exothermic or endothermic? b What is the activation energy for the reverse reaction? c If a catalyst were added to the reaction, how would this affect the activation energy?
Based on the diagram in Exercise 12.83, which of the reactions has the fastest rate? Which has the slowest rate?
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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.
The activation energy for the reaction NO2(g)+CO(g)NO(g)+CO2(g) is 125 kJ/mol, and E for the reaction is 216 kJ/mol. What is the activation energy for the reverse reaction [NO(g) + CO2(g) + NO2(g) + CO(g)]?
. What does the activation energy for a reaction represent? How is the activation energy related to whether a collision between molecules is successful?
In general, can we predict the effect of doubling the concentration of A on the rate of the overall reaction A+BC? Can we predict the effect if the reaction is known to be an elementary reaction?
Bacteria cause milk to go sour by generating lactic acid. Devise an experiment that could measure the activation energy for the production of lactic acid by bacteria in milk. Describe how your experiment will provide the information you need to determine this value. What assumptions must be made about this reaction?