The following elementary steps have been proposed to explain the gas-phase decomposition ofnitrous oxide (N2O).(1)(2)N20N20N2++N2+O2What is the overall reaction for this decomposition? Identify any intermediates.What are the rate laws for the elementary steps?If the experimental rate law is rate = k[N2O][O] which step is the rate-limiting step?The rate constant for a certain second order reaction is 0.0346 s -1 at 25 °C and 0.71 s 1 at 77 °C.What is the energy of activation for this reaction?

The following elementary steps have been proposed to explain the gas-phase decomposition o itrous oxide (N2O). (1) (2) N20 N20 N2 + + N2 O2 What is the overall reaction for this decomposition? Identify any intermediates. What are the rate laws for the elementary steps?

The following elementary steps have been proposed to explain the gas-phase decomposition o itrous oxide (N2O). (1) (2) N20 N20 N2 + + N2 O2 What is the overall reaction for this decomposition? Identify any intermediates. What are the rate laws for the elementary steps?

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

A reaction mechanism has the following proposed elementary steps: Step 1: A ⇌ B + C Step 2: A + B → D Step 3: 2 A + D → C + E Which of the following equations would represent the overall reaction for this mechanism? Which species are intermediates in this reaction? Which of the following would be the correct elementary rate law for Step 1? Which of the following would be the correct elementary rate law for Step 2? Which of the following would be the correct elementary rate law for Step 3? If Step 1 is the rate-limiting step, what would the proposed rate law for this mechanism be? If Step 2 is the rate-limiting step, what would the proposed rate law for this mechanism be?
A mechanism for the gas phase reaction of fluorine with chlorine dioxide that is consistent with the observed rate law is: step 1 slow: F, + CIO, → FCIO2 +F step 2 fast: F+ CIO, → FCIO2 (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. + + (2) Which species acts as a catalyst? Enter formula. If none, leave box blank: (3) Which species acts as a reaction intermediate? Enter formula. If none, leave box blank: (4) Complete the rate law for the overall reaction that is consistent with this mechanism. (Use the form k[A]™[B]"... , where 'l' is understood (so don't write it) for m, n etc.) Rate =
At a certain temperature the rate of this reaction is second order in H₂CO3 with a rate constant of 2.44M *S : H₂CO3(aq) → H₂O (aq) + CO₂ (aq) Suppose a vessel contains H₂CO3 at a concentration of 0.840M. Calculate the concentration of H₂CO3 in the vessel 5.60 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 X
The gas phase decomposition of nitrosyl chloride at 400 K NOCI(g)- →NO(g) + ½ Cl2(g) is second order in NOCI with a rate constant of 5.90x10-4 M-1 s1. If the initial concentration of NOCI is 7.40x10-2 M, the concentration of NOCI will be 1.65x10-2 M after seconds have passed.
Bromide ion is oxidized by bromate ion in acidic solution. 5Br (aq) + BrO3 (aq)+ 6H"(aq) → 3Br,(aq) + 3H,O(1) The experimentally determined rate law is Rate = k[Br ][BrO; ]H7? What is the order of reaction with respect to each reactant species? What is the overall order of the reaction? Br order: O first order O second order O third order O fourth order O fifth order BrO3 order: O first order second order O third order
What is the value of the rate constant for the reaction whose kinetics are described by the following rate law if the initial concentration of reactants A and B are 0.10 M and 0.20 M, respectively, and the initial reaction rate is 3.2 x 105 M/s? Rate k [A]2 [B]3 %3D O 3.9 x 104 M 4s-1 O 0.40 M4s1 O 0.25 M-4s1 O 2.50 M4s-1 O 2.6 x 105 M-4s1
A: Consider the following reaction: N2H5+ + 4 Fe(CN)63- --> N2(g) + 5 H+ + 4 Fe(CN)64- Based on just this information, which species concentration(s) could most likely be in the rate law? (Check ALL correct answers.) Group of answer choices Fe(CN)64- Fe(CN)63- N2H5+ N2(g) H+ B: Consider the following reaction: 2 C19H16O --> C38H32O2, also written as: 2 Monomer --> Dimer Given the following kinetics plot, what is the rate order with respect to Monomer disappearance? Group of answer choices 2nd 3rd Zero 1st
2
For the elementary process, CH3Cl(g) + Cl(g) CH3(g) + Cl2(g), the rate constant increases by a factor of 23.00 when the temperature is raised from 298K to 320K. The value of the gas constant is R = 8.314 J/mol-K. What is the activation energy for this reaction?
What is the rate law for the following reaction? OH O Rate = k [CSH15 OH H2 SO4 ORate = k CSH15 OH [H20] ORate = k[CsH14 ORate = k[C3H15 OH
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__
Suppose also k₁<