Identify the overall rate law for a reaction that has the following mechanism:Step 1 - Fast 0, N2H2=02N2H¯ + H*Step 2 - Slow O2NH¯ → N2O+ OH¯Step 3 - Fast H* + OH→ H,OO ratek[O2 N2 H¯]°O ratek[02 N2 H-][H+]rate[02 N2 H2]k-[H*]rate =k (02 N2 H-]

Answered: Image /qna-images/answer/675a8a82-4db6-4d11-85f9-44afeea84a77.jpg

Identify the overall rate law for a reaction that has the following mechanism: Step 1 - Fast 0, ,H2=02N2H¯ + H* Step 2 - Slow 02 N2H¯ → N20+ OH Step 3 - Fast H* + OH → H20 O rate k[O2 N2 H-] %3D O rate = k[02 N2 H-] [H+] [02 N2 H2] rate k- [H*] O rate = k [O2 N2 H¯]

Identify the overall rate law for a reaction that has the following mechanism: Step 1 - Fast 0, ,H2=02N2H¯ + H* Step 2 - Slow 02 N2H¯ → N20+ OH Step 3 - Fast H* + OH → H20 O rate k[O2 N2 H-] %3D O rate = k[02 N2 H-] [H+] [02 N2 H2] rate k- [H*] O rate = k [O2 N2 H¯]

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

Please answer the question
What is the half-life for a particular reaction if the rate law is rate = (1221 M*min-1)[A]° and the initial concentration of A is 0.250 M?
) Consider the following reaction and data: ??(?) + ??(?) ⟶ ?(?)Determine the rate law for this reaction Calculate the rate constant
Here we compare the first order and second order reaction based on Integrative rate laws. Reaction 1: A first order reaction (A à products) has the rate constant k = 0.483 min-1 (Rate = k[A]), and the initial concentration of reactant A is 0.800 M. Reaction 2: A second order reaction (B à products) has the rate constant k = 0.483 M-1 min-1 (Rate = k[B]2), and the initial concentration of reactant B is 0.800 M. Which of the following statements is true about these two reactions? Choose one option only Options: a. Reaction 1 will take less time to change the reactant concentration from 0.800 M to 0.400 M than Reaction 2 will. b. Reaction 2 will take less time to change the reactant concentration from 0.800 M to 0.400 M than Reaction 1 will. c. Reaction 1 and Reaction 2 will take the same amount of time to change the reactant concentration from 0.800 M to 0.400 M. d. None of the above
Identify the order of the following reactions H Instructions Categorize the following rate laws with corresponding overall order of the reaction. F G E A B C D Rate = K[CO₂] Rate = k Rate = K[HC]2 Rate = K[NO]2[0₂] Rate = K[NO2][F2] Rate = K[SO3] Rate = K[H₂][NO]2 Rate = K[SO₂Cl₂] Which of the reaction(s) are first-order reaction(s)? Select all that apply. Incorrect will be penalized. choices 0000 I FOU EA 000 Which of the reaction(s) are second-order reaction(s)? Select all that apply. Incorrect choices will be penalized. 000000 IVO E CA
Consider this reaction: 2N,0, (e) - 2N,0, te +0,e) At a certain temperature it obeys this rate law. rate - (8.45 M[N,0, %3D Suppose a vessel contains N,O, at a concentration of 0.460M. Calculate how kong it takes for the concentration of N,O, to deorease to 0.0874M. You may assume no other reaction is important Round your answer to 2 significant digits.
I could use help with #2
Consider the following reaction. From the given choices of intermediates, choose the 5 related to this reaction and put them in order to describe the complete mechanism (all the steps involved) for this reaction.
Consider the following chemical reaction involving hydrogen gas and NO. The value of the specific rate constant at this temperature is H2(g) + 2 NO(g) → N20(g) + H2O(g) (MTS 2/17/2018) Experiment Initial [NO] (M) Initial [H2]_(M). Initial Rate (M•s-1) 1 0.30 0.35 2.835 x 10-3 2 0.60 0.35 5.670 x 10-3 3 0.60 0.70 2.268 x 10-2
6. Given the reaction: CH3(CO)CH3 (M) | B(M) 0.010 0.010 CH3(CO)CH3 + I2 + H* → CH3(CO)CH2I + HI H* (M) Rate (M/s) 0.010 3.0 x 10-4 0.010 6.0 x 10-4 0.020 6.0 x 104 0.020 2.4 x 10-3 0.040 4.8 x 10-3 0.010 6.0 x 104 0.010 0.020 0.010 0.040 0.040 0.020 0.020 0.040 0.020 0.040 a. Determine the reaction order for each reactant. b. Solve for the rate constant, k, and the appropriate units. c. Write the rate law for the reaction, including a value for k. d. Solve for the rate of the reaction if there are 1.25 M of CH3(CO)CH3, 2.25 M of I2, and 3.25 M H*.
What is the rate constant of a first-order reaction when 20.0% of a reactant remains after 48.0 s? | 1/s 1 3 4 C 7 8 9 +/- х 100
mm