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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Suppose you have a reaction between A and that forms product C: A B C and that A and B are both added at equal concentrations to a reaction vessel. At the end of 120 min you find that the concentration of A is just 30% of what it was originally. You have previously determined that the reaction proceeds as first order in [A] and zero order in [B]. How much of the initial amount of A will remain at the end of 240 min? 9.00 % O 17.6% O 0.000% O 14.2%
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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
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
for the reaction between nitrogen monoxide and chlorine to produce nitrosyl chloride 2NO + Cl2 --> 2NOCl it is found that tripling the concentration of both reactants increases the rate by a factor of 27. if only the concentration of chlorine is tripled the rate increases by a factor of 3. give order of this reaction with respect to NO and determine the rate law for the reaction
Consider the overall reaction 2A + B ⇌ 2C(g) with proposed mechanism for this reaction: A + B ⇌ C + D (slow) A+D ⇌ C (fast)What is the rate law for this proposed mechanism?
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 =