A reaction mechanism is defined as the sequence of reaction stepsthat define the pathway from reactants to products. Each step in amechanism is an elementary reaction, which describes a singlemolecular event of usually one or two molecules interacting.Part AThe rate law for an overall reaction is the rate law for the slowest stepin the mechanism, which is directly related to the stoichiometriccoefficients of the reactants.What is the rate law for the following mechanism in terms of the overall rate constant k?Step 1:Step 2: B+ CC ( fast)+ D (slow)A +BThe exception to this rule occurs when the slowest step containsintermediates. In these cases, the slowest step is usually preceded byan equilibrium step, which can be used to substitute for theintermediates in the overall rate law.Express your answer in terms of k and the necessary concentrations (e.g., k*[A]^3* [D]).• View Available Hint(s)Hνα ΑΣφ?rate =

Rate law of chemical reaction is an equation that provides relationship between rate and…

Part A What is the rate law for the following mechanism in terms of the overall rate constant k? Step 1: A+B - c (fast) Step 2: B+C → D (slow) Express your answer in terms of k and the necessary concentrations (0.g., k*[A]^3•[D]). > View Available Hint(s) ? rate =

Part A What is the rate law for the following mechanism in terms of the overall rate constant k? Step 1: A+B - c (fast) Step 2: B+C → D (slow) Express your answer in terms of k and the necessary concentrations (0.g., k*[A]^3•[D]). > View Available Hint(s) ? rate =

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

For the reaction H2(g) + C2H4(g) ⟶⟶C2H6(g) A series of experiments were conducted as sown in the Table. If the rate law were found to be : rate = k[H2][C2H4] what is the missing initial rate (marked with a "?" in the Table)?
Using the following data below for the generic reaction A + B --> 2C + D , which obeys the rate equation d[D]/dt=k[A]α[B]β [A] (M) [B] (M) d[D]/dt (M/s) 0.300 0.300 1.31×10−5 0.600 0.300 3.69×10−5 0.300 0.600 1.85×10−5 a. What are the orders with respect to A and B (α,β)? What is the overall reaction order? b. What is the value of the rate constant k? Be sure to include units. c. Collecting concentration vs. time data would be another possible method to determine k. Describe and sketch the way you would plot these data to obtain a linear relationship, and how you would determine k based on this plot.
Step 2: NO2 + F→ NO₂F (fast) (a) Write a rate law for the overall reaction that is consistent with the proposed mechanism. Rate = k [No₂][F] (b) On the incomplete reaction energy diagram below, draw a curve that shows the following two details. The relative activation energies of the two elementary steps The enthalpy change of the overall reaction Energy 2 NO2 + F2 (a) OK Reaction Progress
Consider the following reaction: 12 (g) + H2 (g) --> 2 HI (g). Given the mechanism below, determine the rate law for the equation. Note: input the rate law following the format rate-k[A]2[B2] with no spaces don't worry about formatting upper or lower case. 1₂ (g) 21 (g) (fast) H₂ (9)+21 (g) → 2HI (g) (slow)
It has been found that DDT in the soil decomposes by a first-order reaction with a half-life of 12.0 years. How long would it take DDT in a soil sample to decompose from a concentration of 435 ppbm (parts per billion by mass) to 15 ppbm? | yr 1 2 3 4 5 6. C 7 8. 9. +/- х 100 CO
Question 4 Calculate the frequency factor (A). Studies have shown that the reaction occurs via the following mechanism. ki Cl2O4 k-1 Step 1: 2 Cl02 (fast equilibrium) k2 Step 2: C2O4 + OH- → ClO;¯+HCIO2 (slow) k3 Step 3: HCIO2 + OH → ClO2¯+H2O (fast) Question 5: Identify the intermediate/s and the rate-determining step. ki 2 ClO2 2 C2O4 k-1 Step 1: (fast equilibrium) k2 → ClO3¯+HC1O2 Step 2: C204 + OH- (slow) k3 Step 3: HC1O2 + OH- ClO2- + H2O (fast) Question 6 Is the proposed mechanism consistent with the experimentally determined rate law? Show your solution to justify your answer. ki 2 ClO2 2 C2O4 k-1 Step 1: (fast equilibrium) k2 Step 2: C204 + OH- → ClO3¯+ HCIO2 (slow) k3 Step 3: HCIO2 + OH- → ClO2-+ H2O (fast) Question 7 Draw the transition state for Step 3. Identify the bond/s forming/breaking.
The integrated rate law is an equation that describes the concentration of a reactant over time (t). The integrated rate law comes in different forms depending on the reaction order. The rate laws below are given for a simple general reaction A-products Order 0 1 2 Integrated rate law [A] = -kt+ [A]o In[A] = − kt+In[A]o =kt+ [A]o Linear graph Slope [A] vs. t -k In[A] vs. t -k V vs. t k
rate = k(NO2)(F2) b) Calculate the value of the rate constant, kk. Express your answer in liters per mole per second to three significant figures. c) What is the overall order of the reaction?
The decomposition of nitramide, O₂NNH,, in water has the chemical equation and rate law [O₂NNH₂] [H+] O₂NNH, (aq)- -N₂O(g) + H₂O(1) A proposed mechanism for this reaction is 1.0,NNH, (aq) = O,NNH(aq) + H+ (aq) (fast equilibrium) rate = k 2.0, NNH (aq) N₂O(g) + OH- (aq) (slow) 3. H(aq) + OH-(aq) H₂O(l) (fast) What is the relationship between the observed value of k and the rate constants for the individual steps of the mechanism? k₂ Answer Bank k_ k3 k
Please don't provide handwritten solution...
The decomposition reaction of ammonia gas (NH3) into hydrogen gas (H2) and nitrogen (N2) with a Pt catalyst is a zero order reaction at a temperature of 1130 K (i) rate of reaction = rate constant,(ii) reaction rate depends on ammonia concentration,(iii) the rate of decomposition of ammonia becomes constant when the ammonia has completely reacted,(iv) an increase in gas pressure will change the rate of the reaction. A. (ii) and (iv)B. (i) and (ii)C. (i), (ii) and (iii)D. (ii), (iii) and (iv)E. (i), (iii) and (iv)
?.):)6)6:)6:)6):7