The mechanism for the reaction described byNO₂(g) + CO(g) → CO₂(g) + NO(g)is suggested to bek1(1) 2NO₂(g) →→→ NO₂(g) + NO(g)k₂2(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).2rate of CO₂(g) production = k₁ [NO]²

Steady state approximation is applied on the intermediate species. According to ssa, rate of…

The mechanism for the reaction described by NO₂(g) + CO(g) CO₂(g) + NO(g) is suggested to be k₁ (1) 2 NO₂(g) → NO3(g) + NO(g) k₂ (2) NO3(g) + CO(g) NO₂(g) + CO₂(g) Assuming that [NO3] is governed by steady-state conditions, derive the rate law for the production of CO₂(g). rate of CO₂(g) production = k₁ [NO]²

The mechanism for the reaction described by NO₂(g) + CO(g) CO₂(g) + NO(g) is suggested to be k₁ (1) 2 NO₂(g) → NO3(g) + NO(g) k₂ (2) NO3(g) + CO(g) NO₂(g) + CO₂(g) Assuming that [NO3] is governed by steady-state conditions, derive the rate law for the production of CO₂(g). rate of CO₂(g) production = k₁ [NO]²

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...

See similar textbooks

Similar questions

The reaction 2H2(g) + 2ClO(g) --------> 2H2O(g)+ Cl2(g) is first-order in H2 and second-order in ClO. What is the rate law?
The overall reaction 2 NO (g) + O2 (g) → 2 NO2 (g) is believed to take place in the following steps: 2 NO (g) N2O2 (g) (fast) N2O2 (g) + O2 (g) → 2 NO2 (g) (slow) Obtain a rate expression that corresponds to this proposed mechanism.
8. For the overall reaction: 2NO (g) + O2 (g) → 2NO2 (g), the following mechanism has been proposed: (1) 2NO (g) = N2O2 (g) (2) N2O2 (g) + O2 (g) → 2 NO2 (g) a) Determine the rate law expression for this reaction. The steady-state approximation can be used for the N2O2 intermediate. b) Simplify the rate law expression if the rate constant for reaction (2) is much larger than that for the reverse reaction (1).
Consider the following mechanism for the reduction of nitric oxide: H₂(g) + 2NO(g) → N₂O(g) + H₂O(g) H₂(g) + N₂O(g) → N₂(g) + H₂O(g) Write the chemical equation of the overall reaction: Are there any intermediates in this mechanism? If there are intermediates, write down their chemical formulas. Put a comma between each chemical formula, if there's more than one. O yes Ono (1) (2) X 00 e 4
One of the reactions that occurs in polluted air in urban areas is 2NO2(g) + O3(g) –→N2O5(g) + O2(g). Assume that a species with the formula NO3 is involved in the mechanism, and the observed rate law for the overall reaction is rate = k[NO2][O3]. Propose a mechanism for this reaction that includes the species NO3 and is consistent with the observed rate law. NO2(g) + O3(g) – NO3(g) + O2(g) (fast) NO3(g) + NO2(g) → N2O5(g) (slow) NO2(g) + O3(g) – NO3(g) + O2(g) (fast) 4NO3(g) 2N2O5(g) + O2(g) (slow) NO2(g) + O3(g) –→ NO3(g) + O2(g) (slow) NO3(g) + NO2(g) → N2O5(g) (fast) NO2(3) + O3(g) → NO3(g) + O2(g) (slow) 4NO3(3) → 2N20O5(g) + O2(g) (fast)
9) The following three-step mechanism has been proposed for the reaction of chlorine and chloroform. rate constants 1) Cl2(g) ↔ 2 Cl(g) Keq1 =2.5 k1 = 5.5 x 103 sec-1 2) Cl(g) + CHCl3(g) → HCl(g) + CCl3(g) k2 = 2.4 x 10−2 M-1sec-1 3) CCl3(g) + Cl(g) → CCl4(g) k3 = 3.6 x 102 M-1sec-1 a) Write the equation for the overall reaction. __a__ b) Write the rate law for the overall reaction. __b__ c) Calculate the rate constant for the overall reaction (include units) __c__
Consider the following reaction for chlorine reacting with chloroform, Cl2 (g) + CHCIl3 (g) HС (g) + СCla (g) a) based on the initial rate data provided (in the table below), determine the rate law for this reaction. b) The following is a proposed mechanism for this reaction. Cl2 (g) = 2 CI (g) CI (g) + CHCI: (g) → HCI (g) + CCl: (g) (slow) CCl: (g) + CI (g) > Сle (g) (fast equilibrium) (fast) Is this an acceptable mechanism based on the rate law you determined in part a? answer should be Yes/No to "is this an acceptable mechanism") Initial Rate [CI,] [CHCI3] 0.00253 | 0.2 0.3 A) Yes 0.00759 0.2 0.9 B) No 0.00506 0.8 0.3
The recombination reaction 2 HO₂(g) → H₂O2(g) + O₂(g) has a second-order rate constant of 1.8E9 M1 s1. Calculate the half-life of the reaction if the initial concentration of HO₂(g) is 1.7E-11 M. Note: the coefficient 2 in the reaction means that the integrated rate law for this reaction is: 1/c = 1/co+2kt Include at least 3 significant figures in your answer. Show Transcribed Text
The decomposition of ethylene oxide (CH₂)₂O(g) → CH₄(g) + CO(g) is a first order reaction with a half-life of 58.0 min at 652 K. The activation energy of the reaction is 218 kJ/mol. Calculate the half-life at 617 K.
The decomposition of ethylene oxide (CH₂)₂O(g) → CH₄(g) + CO(g) is a first order reaction with a half-life of 58.0 min at 652 K. The activation energy of the reaction is 218 kJ/mol. Calculate the half-life at 623 K.
Consider the reaction, A + B + C => D, which is found to be first order in A, first order in B and first order in C. Which step of the proposed mechanism must be slow in order to agree with this rate law? 1. A(g) + B(g) => X(g) 2. X(g) + C(g) => Y(g) 3. Y(g) => D(g) A. 1 B. only 3 C. Either 2 or 3 D. only 2
A proposed mechanism for the decomposition of hydrogen peroxide consists of three elementary steps: (1) H₂O2(g) →>> 2OH(g) (2) H₂O2(g) + OH(g) → H₂O(g) + HO₂(g) (3) HO₂(g) + OH(g) → H₂O(g) + O₂(g) If the rate law for the reaction is first order in H₂O2, which step in the mechanism is the rate-determining step? O Step 1 O None of the steps O Step 3 O Impossible to determine Steps 1 and 2 O All of the steps O Step 2 Hint: The slowest step in a mechanism determines the rate law. From each elementary reaction we can write a rate-law expression. Submit Question