A certain chemical reaction 2A B + C is proposed to occur in three elementary steps: Step 1: A = C +E (fast) Step 2: A + E =B (slow) Which one of the following rate laws is consistent with the proposed mechanism? K[A][C] A. Rate = B. Rate = k[A][B]-1 %3D C. Rate = k[A] D. Rate = k[A]? %3D E. Rate = k[A]°[C]-1 %3D

A certain chemical reaction 2A B + C is proposed to occur in three elementary steps: Step 1: A = C +E (fast) Step 2: A + E =B (slow) Which one of the following rate laws is consistent with the proposed mechanism? K[A][C] A. Rate = B. Rate = k[A][B]-1 %3D C. Rate = k[A] D. Rate = k[A]? %3D E. Rate = k[A]°[C]-1 %3D

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 H2(g) + I2(g) → 2HI(g) may occur by the mechanism shown above. What is the rate law predicted by the mechanism?
Copy of Consider a reaction that has the form aA -> Products At a particular temperature, a concentration versus time data was collected. A plot of [A] vers would be a correct representation of the differential rate law: 1 d[A] = k [A] a dt 1 d[A] = k a dt 1 d[A] = k[A] a dt 1 d[A] = k dt
5. The reaction A →B+C is known to be first order in A. Below are data showing the concentration of A as a function of reaction time. Time, min [A], M 5.00 x 10-2 4.30 x 10-2 5 10 3.70 x 10-2 2.74 x 10-2 1.51 x 10-2 20 40 1.12 x 10-2 8.26 x 10-3 50 60 (a) What is the average rate of reaction between 5 and 20 min? Report the units as well as the numbers. (b) Plot the data above, showing the concentration of A as a function of the time. From your graph, determine the instantaneous rate of reaction at 40 min. Report the units as well as the numbers. (c) Plot In [A] versus time. Estimate the rate constant for this first-order reaction from your graph. Report the units as well as the numbers.
The following are initial rate data for: A + 2B - C + 2 D Experiment Initial [A] Initial [B] Initial Rate 1 0.10 0.10 0.300 0.20 0.10 0.600 3 0.10 0.20 1.200 What is the rate law? The rate law is Rate = k[A]?[B]1. The rate law is Rate = k[A]?[B]*. The rate law is Rate = k[A]?[B]°. The rate law is Rate = k[A]°[B]?. The rate law is Rate = k[A]²[B]².
For a reaction with the rate law below: Rate = k[A]? %3D a plot of In[A] vs. time gives a straight line. a plot of 1/[A] vs. time gives a straight line. a plot of 1/[A] vs. 1/time gives a straight line. O a plot of [A] vs. time gives a straight line. O a plot of log [A]o/[A] vs. 1/time gives a straight line. A Moving to another question will save this response. esc 20 F3 F1 F4 $4 1. 2. 4 Q W R. # 3
Q1
General Chemistry 4th Edition McQuarrie • Rock • Gallogly dUniversity Science Books presented by Macmillan Learning The reaction C,H¿ (g) → 2 C,H¿(g) has an activation energy of 262 kJ/mol. At 600.0 K, the rate constant, k, is 6.1 × 10-8 s-!. What is the value of the rate constant at 840.0 K? k =
The rate constant for the reaction is 0.200 M-! · s-! at 200 °C. A products If the initial concentration of A is 0.00780 M, what will be the concentration after 105 s? [A] = M * TOOLS x10
Use average bond enthalpies (linked above) to calculate the enthalpy change for the following gas-phase reaction. C2H4(g) + Br2(g) CH,BRCH,Br(g) To analyze the reaction, first draw Lewis structures for all reactant and product molecules. • Include all valence lone pairs in your answer. • Draw the reaction using separate sketchers for each species. One molecule per sketcher, please. Separate multiple reactants and/or products using the + sign from the drop-down arrow. Separate reactants from products using the If you have to draw H,, draw H-H. • Be sure that your structural equation is balanced. symbol from the drop-down menu.
A) In the proposed reaction mechanism below, the intermediate product is: A). NO(g) B). N2O2(g) C). H2(g) D). N2O(g) B) The rate expression for a particular reaction is rate = k[A][B]^2. If the initial concentration of B is increased from 0.10M to 0.30M, the initial rate will increase by which of the following factors A) 2 B) 3 C) 6 D) 9
The following reaction has rate law r = k[C4H6] 2 , where k = 0.014 M-1 s -1 What is the concentration of C4H6 (in M) after 3.0 hours, if [C4H6]o = 0.025 M? A. 0.0052 M B. 0.024 M C. 0.012 M D. 0.0060 M
4. Given: A +B O C Rate ( M sec ') 4.0X 10 -5 4.0 X 105 16 X 10-5 [] 0.1 [B] 0.1 0.1 0.2 0.2 0.1 Determine the rate law. Calculate the rate constant. Determine the rate when [A] = 0.05 and [B] = 0.10