Part A In the gas phase, the reaction between O2 and NO produces NO2. Define the reaction rate in terms of the disappearance of O2, and use the steady-state approximation to determine the rate law predicted by this mechanism. O2 + 2NO NO2 The reaction is proposed to occur via the following mechanism: Drag the appropriate labels to their respective targets. 2NO N2O2 O2 + N2O2 2NO2

Part A In the gas phase, the reaction between O2 and NO produces NO2. Define the reaction rate in terms of the disappearance of O2, and use the steady-state approximation to determine the rate law predicted by this mechanism. O2 + 2NO NO2 The reaction is proposed to occur via the following mechanism: Drag the appropriate labels to their respective targets. 2NO N2O2 O2 + N2O2 2NO2

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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For the reaction 3O2(g) + 4NO(g) → 2N2O5(g) the rate of change in concentration of O2, Δ[O2]/Δ t = 0.48 mol/L*sec. What is the rate of change of NO and what is the rate of change of N2O5? Show your calculations.
The reaction between N2O5 and water$$N2O5(g)+H2O(g)2HNO3(g)is a source of nitric acid in the atmosphere. The reaction is first order in each reactant. Write the rate law for the reaction.
8. a) Starting from the rate law for the second order reaction below, derive the relationship between half- life, rate constant, and initial concentration. 2A → B 8. b) Draw the potential energy diagrams (qualitatively) for the following reaction mechanisms. Assume that all intermediates are higher energy than their respective reactant states, and that the product state is lower in energy than the reactant state. Mechanism 1: 03 + NO → 02 + NO3 (slow) 0 + 03 → 2 02 (fast) NO3 + NO → 2 NO2 (fast) Mechanism 2: 03 2 02 +0 (fast) NO + 0 → NO2 (slow) Mechanism 3: 03 + NO → 02 + NO2 (slow)
The balanced chemical equation and rate law for the reaction between NO(g) and H2(g) at a particular temperature are 2NO(g) + 2H₂(g) → N₂(g) + 2H₂O(g) Rate = k[NO] [H₂] What is the reaction order with respect to nitric oxide AND the overall order of the reaction? 2,3 2,4 4,3 1,4 0,2
1) NO(g) + O2 (g) >< NO3 (g) 2) NO3(g) + NO(g) > < 2NO2(g0 for the reaction mechanism given, what is the rate law for each elementary equation? What is the rate law for the overall reaction if the mechanism is correct?
An energy diagram showing two peaks suggests that there are two steps and three transition states in the reaction mechanism. Select one: O True O False Given a reaction with an activation energy of 2.3 x 104 J/mol. The rate constant will increase by a factor of when the reaction temperature is increased from 200 °C to 250 °C. O 2.42 O 2.81 O 1.58 O 1.75 For the complete neutralization reaction between a 1 M strong acid and a 1 M strong base of equal initial volumes that is marked by a temperature rise, the entropy of neutralization is positive (ASn > 0) whereas the Gibbs free energy is negative (AGxn < 0). Select one: O True O False
9. The reaction 3C A + 2B occurs in one step in the gas phase. In each blank below, write the exponent of the concentration in the FORWARD rate law or write none if that concentration does not appear in the rate law. [A] ........... [B] .......... [C] ...........
9
A. Consider the following proposed mechanism for the production of chlorine dixoide from chlorine and ozone. Draw a reaction coordinate diagram for this reaction. Label reactants, products, transition states, intermediates, and activation energy on your sketch. Assume the reaction is endothermic. NOTE: CI is chlorine, not Carbon lodide Overall: Cl₂ (g) + 203 (g) → 2 CIO₂ (g) + O₂ (g) Step 1: Cl₂ (g) → 2 Cl (g) fast Step 2: Cl (g) + Os (g) CIO₂ +O fast Step 3: O (g) + O3 (g) → 202 (g) fast Step 4: Cl (g) + O2 (g) → CIO2 (g) slow
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Using an integrated rate law for a first-order reaction At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.141 s¯¹: H₂CO3(aq) → H₂O (aq) + CO₂ (aq) Suppose a vessel contains H₂CO3 at a concentration of 0.290M. Calculate the concentration of H₂CO3 in the vessel 4.40 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 X Ś
The mechanism for the reaction described by NO₂(g) + CO(g) → CO₂(g) + NO(g) is suggested to be k₁ (1) 2 NO₂(g) NO₂(g) + NO(g) k₂ (2) NO3(g) + CO(g) → NO₂(g) + CO₂(g) Assuming that [NO] is governed by steady-state conditions, derive the rate law for the production of CO₂ (g). rate of CO₂ (g) production =