Example: For the following reaction 2H2 (g) + 2NO(g) → N2 (g) + 2H2O(g) the experimentally determined rate law is rate = k [H2][NOJ? For each of the following two mechanisms, state whether it is possible or not possible for it to describe the overall reaction. Show all of your work Mechanism I Mechanism II H2(g) + NO(g) → H;O(g) + N(g) (slow) H2 (g) + 2NO(g) → H¿O(g) + N¿O(g) (slow) N(g) + NO(g) → N2 (g) + O(g) (fast) N2O(g) + H2 (g) → N2 (g) + H2O(g) (fast) O(g) + H2 (g) → H¿O(g) (fast)

Example: For the following reaction 2H2 (g) + 2NO(g) → N2 (g) + 2H2O(g) the experimentally determined rate law is rate = k [H2][NOJ? For each of the following two mechanisms, state whether it is possible or not possible for it to describe the overall reaction. Show all of your work Mechanism I Mechanism II H2(g) + NO(g) → H;O(g) + N(g) (slow) H2 (g) + 2NO(g) → H¿O(g) + N¿O(g) (slow) N(g) + NO(g) → N2 (g) + O(g) (fast) N2O(g) + H2 (g) → N2 (g) + H2O(g) (fast) O(g) + H2 (g) → H¿O(g) (fast)

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

Can someone please help with question 1b
For the gas phase decomposition of t-butyl alcohol, (CH3)3COH(CH3)½C=CH, + H,O the rate constant in s has been determined at several temperatures. When In k is plotted against the reciprocal of the Kelvin temperature, the resulting linear plot has a slope of -3.30x104 K and a y-intercept of 33.8. The value of the rate constant for the gas phase decomposition of t-butyl alcohol at 806 K is ]s!.
For the following reaction: H2(g) + ICl(g) ----> HI(g) + HCl(g) slow HI(g) + ICl(g) ---> I2(g) + HCl(g) Write the rate law.
Consider the following multistep reaction: C+D = CD (fast) CD+D →CD2 (slow) CD2 +D→CD3 (fast) C+ 3D →CD3 (overall) Based on this mechanism, determine the rate law for the overall reaction. Express your answer in standard MasteringChemistry format. For example, if the rate law is k[C]° [D]? type k* [C]^3* [D]^2. • View Available Hint(s)
Suppose the reduction of nitric oxide proceeds by the following mechanism: step elementary reaction rate constant 1 H, (g) + 2NO (g) → N,0 (g)+ H,0 (g) k1 H, (g) + N,0 (g) → N2 (g) + H20 (g) k2 Suppose also k, « k,. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. rate = k|| Note: your answer should not contain the concentrations of any intermediates.
rate constant 1 H₂(g) + 2NO(g) N₂O(g) + H₂O(g) k₁ 2 H₂(g) + N₂O(g) → N₂(g) + H₂O(g) k₂ Suppose also k₁«k₂. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical reaction. rate = k Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of k1, K₂, and (if necessary) the rate constants k-1 and k-2 for the reverse of the two elementary reactions in the mechanism. step elementary reaction t k = A 00 X
A possible mechanism for the reaction described by: CO(g) + Cl2(g) → COCl2(g) Identify any intermediate species + write the rate law for each step. *I'm confused on how to identify intermediate species and why the rate law for 2 = k2[Cl]2 Answers: Cl(g) and COCl(g) are intermediate species. The rate laws are k1[Cl2], k2[Cl]2, k3[Cl][CO], and k4[COCl][Cl2], respectively.
A possible mechanism for the next decomposition reaction is A(g) ⇄ 2B(g) + C (fast equilibrium) C + A(g) → 2B(g) (slow) What is a rate law that is consistent with this mechanism?
The rate law for: Cl2(g) + CHCl3(g) → HCl(g) + CCl4(g) is rate = k [Cl2]1/2 [CHCl3]3/4 The units for the rate constant are: M−1sec−1 M−1/4sec−1 sec−1 M−3/4sec−1 M−2sec−1
O KINETICS AND EQUILIBRIUM Writing the rate law implied by a simple mechanism H₂(g) + ICI(g) - 1 HI(g) + HCl(g) k₁ 2 HI(g) + ICl(g) 1₂(g) + HCl(g) k₂ Suppose also k₁«k₂. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of k₁, K₂, and (if necessary) the rate constants k.₁ and k-2 for the reverse of the two elementary reactions in the mechanism. Explanation Check rate = k0 = 0 k = JUL 16 L tv W MacBook Air ローロ 00 X 0- © 2023 McGraw Hill LLC. All Rights Reserved. Terms of 70
The reaction 2H2(g) + 2NO(g) ----> 2H2O(g) + N2(g) is a first-order in H2 and second order in NO. What is the rate law
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