Step 1:(slow)Step 2:(fast)O = CIThe particle models shown above represent a proposed two-step mechanism for the destruction of ozone(03) in the upper atmosphere.Based on the models, which of the following represents a species that acts as a catalyst for thereaction?

When chlorofluorocarbons, CFCl3 released in atmosphere, it will depleted the ozone layer , O3 in…

Step 1: (slow) Step 2: (fast) O = CI = 0 The particle models shown above represent a proposed two-step mechanism for the destruction of ozor (03) in the upper atmosphere. Based on the models, which of the following represents a species that acts as a catalyst for the reaction?

Step 1: (slow) Step 2: (fast) O = CI = 0 The particle models shown above represent a proposed two-step mechanism for the destruction of ozor (03) in the upper atmosphere. Based on the models, which of the following represents a species that acts as a catalyst for the reaction?

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A reaction is performed to study the oxidation of arsenate ion by cerium(IV) ion in aqueous solution: + 2 Ce** + H20 AsO, + 2 Ce3+ + 2 H* The following reaction rate data was obtained in four separate experiments. [Ce**Jo• M [AsO3³ lo, M 3.60x10-2 7.20×10-2 3.60x10-2 7.20×x10-2 Experiment Initial Rate, Ms1 6.89x10-3 1.38×10-2 2.76x10-2 5.52x10-2 1 0.595 2 0.595 1.19 14 1.19 What is the rate law for the reaction and what is the numerical value of k? Complete the rate law in the box below. Remember that an exponent of 'l' is not shown and concentrations taken to the zero power do not appear. Rate = k = M2s!.
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Americium-241 is used in smoke detectors. It has a first order rate constant for radioactive decay of k = 1.6*10-3 yr-1. By contrast, iodine-125, which is used to test for thyroid functioning, has a rate constant for radioactive decay of k = 0.011 day-1. How much of a 1.00 mg sample of iodine-125 remains after 4 days?
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0.1 M of a material has a decomposition rate constant (k) of 2.46×105 M-1 s-1. What equation would you use to calculate the half-life of decomposition?
23. A reaction proceeds by a series of elementary steps as shown below. The activation energy and heat of reaction are shown for each step. Step No. Elementary Step Activation Energy Enthalpy of Reaction 1 АВ — А + %2B, 12 kJ 35 kJ 2 C + B2 → CB, 2.5 kJ -29 kJ 3 АС — А + С 7.5 kJ 21 kJ a) What is the overall equation for this reaction? Show your work. b) What is the heat of reaction for the overall equation? Show your work. c) Which step is the rate determining step and why? d) Using the space provided below, draw and label a potential energy diagram to represent the overall equation in (a). I
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3. The rate equation for the decomposition of N,Os(g) (forming NO2(g)) is: A[NO2]/At = k[N;Os]. The value of k is 5.0 × 104 s-1 for the reaction at a particular temperature. a) Calculate the half-life of N2O5(g) at that temperature. b) How long does it take for [N½O5] to decrease to one tenth of its original value?
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