Name:The half-life of a first-order decomposition reaction is 188 şeconds. If the initial concentration ofreactant is 1.00 M. what is the value of the rate constant?11.a.920.00370.0027b.c.d.0.0053The next three questions refer to the proposed mechanism:Step IStep IIA +B --> C +DA +C --> Dslowfast2ATB -2l12DB 12. What is the molecularity of the first step?unimolecularbimoleculartermolecularab.с.d.quadmolecular13. What would be the overall reaction represented by this mechanism?a A+B --> C + D2 A+B --> 2 C + 2 Db.с.2 A +B --> 2 Dd. 2 A+B --> C + D14. What would you expect the units to be for the rate constant for the overall rate equation?M³s!b. M²s!M's-d. s-la.rate = KCA]? [BJ'с.

All the given questions discuss about the several concepts related to rate laws such as half life,…

Name: 11. The half-life of a first-order decomposition reaction is 188 seconds. If the initial concentration of reactant is 1.00 M, what is the value of the rate constant? 92 a. 0.0037 0.0027 b. c. d. 0.0053 The next three questions refer to the proposed mechanism: Step I Step II A +B --> C + D A +C--> D slow fast 2ATB -2etZD B 12. What is the molecularity of the first step? a. unimolecular b. bimolecular с. termolecular d. quadmolecular 13. What would be the overall reaction represented by this mechanism? a A+B -->C + D b. 2 A+B--> 2 C + 2 D с. 2 A +B --> 2 D d. 2 A+B--> C + D 14. What would you expect the units to be for the rate constant for the overall rate equation? M's b. M's M's a. rate = K CA]? CBJ' с. d. s-l

Name: 11. The half-life of a first-order decomposition reaction is 188 seconds. If the initial concentration of reactant is 1.00 M, what is the value of the rate constant? 92 a. 0.0037 0.0027 b. c. d. 0.0053 The next three questions refer to the proposed mechanism: Step I Step II A +B --> C + D A +C--> D slow fast 2ATB -2etZD B 12. What is the molecularity of the first step? a. unimolecular b. bimolecular с. termolecular d. quadmolecular 13. What would be the overall reaction represented by this mechanism? a A+B -->C + D b. 2 A+B--> 2 C + 2 D с. 2 A +B --> 2 D d. 2 A+B--> C + D 14. What would you expect the units to be for the rate constant for the overall rate equation? M's b. M's M's a. rate = K CA]? CBJ' с. d. s-l

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

9
The kinetics of a gas phase reaction of the form A - Products results in a rate constant of 0.00781 M/min. For this reaction, the initial concentration of A is 0.215 M. min How many minutes will it take for the concentration of A to reach 0.062 1 4 8. 9. +/- étv A FEB 28 MacBook Air DI DD 80 888 F10 F11 F8 F9 F6 F7 F5 F2 F3 F4 F1 3.
Number 4
At a particular temperature, N 20 5 decomposes according to a first-order rate law with a half-life of 3.0 s. If the initial concentration ofN 20 5 is 1.0 х 10 16 molecules/cm what will be the concentration in molecules/cm 3 after 11.5 s? O a. 1.0 × 1016 O b.2.3 × 10-1 O. 7.0× 1014 O d. 3.4 x 101 O e. 2,0 × 1014
A certain reaction is first order in H, and first order in I,. Use this information to complete the table below. Round each of your answers to 3 significant digits. [H.] [1] initial rate of reaction 1.10 M 0.547 M 16.0 M/s I M/s 2.43 M 0.547 M I M/s 2.20 M 0.273 M
5.
I need help with both of the blank spaces with correct significant figures
6. The rate constants for the decomposition of a compound are 6.2 x 10* s' at 45°C and 2.1 x 103 s1 at 55°C. What is the value of the activation energy for this reaction in kJ/mol? А. 1.7 х 10% В. 1.1 x 105 C. 2.5 x 103 D. 2.5 x 104 E. 1.1x 106
The initial rate of a reaction which is first order in A is 2.0 x 106 M/s when the initial concentration is 0.0075 M. What is the first order rate constant (s)? A 2.7 x 10-4 s-1 3.8 x 10-9 M-1 s-1 S C 2.7 x 10-4 M-1 s-1 3.8 x 10-9 s-1
B 8. D Trial 1 2 3 4 [A₂] 0.10 0.20 0.30 0.30 [B] 0.50 0.50 0.05 0.10 An experiment was conducted to determine the rate law for the reaction A2(g) + B(9) A₂B(g). The table above shows the data collected. Based on the data in the table. which statement is correct? Initial rate (Ms-¹) 2.5 x 10 5.0 x 10-4 5.0 × 10-5 1.0 x 10-4 Since the rate law can be expressed as ratek[A₂), tripling the concentration of A2 will cause a 9-fold increase in the rate of the reaction. Since the rate law can be expressed as rate k[A₂][B], doubling the concentrations of A₂ and B will quadruple the rate of the reaction. Since the rate law can be expressed as rate k[A] [B], tripling the concentration of A2 while keeping the concentration of B constant will triple the rate of the reaction. Since the rate law can be expressed as rate=k[A₂][B], doubling the concentration of B while keeping the concentration of A₂ constant will double the rate of the reaction.
A certain reaction is first order in N₂ and second order in H₂. Use this information to complete the table below. Be sure each of your answer entries has the correct number of significant digits. [N₂] 1.59 M 5.93 M 5.10 M H₂] 1.61 M 1.61 M 0.502 M initial rate of reaction 3 7.00 X 10 M/s MIS M/S x10 X Ś
The following data was collected for the reaction 2 Mg + O2 --> 2MgO Determine the order for each reactant and write the rate law. Trial [Mg] (mol/L) [O2] (mol/L) Measured Rate(M/s) 1 .10 .10 2.0x10-3 2 .20 .10 4.0x10-3 3 .10 .20 8.0x10-3 According to this data the order for Mg is Answer (enter a number).