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...

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KINETICS AND EQUILIBRIUM Identifying intermediates in a reaction mechanism Consider the following mechanism for the reduction of nitric oxide: H₂(g) + 2NO(g) → N₂O(g) + H₂O(g) H₂(g) + N₂O(g) → N₂(g) + H₂O(g) Write the chemical equation of the overall reaction: Are there any intermediates in this mechanism? If there are intermediates, write down their chemical formulas. Put a comma between each chemical formula, if there's more than one. ☐ yes no (1) (2) ローロ 00 09 0.0.... X Ś 0/3
The reaction A + 2 B → C has the rate law rate = k[A][B]. By what factor does the rate of reaction increase when both [A] and [B] are doubled? What is the half-life for a particular reaction if the rate law is rate = (1301 min⁻¹)[A]? Identify the molecularity of the elementary reaction below: 2NO(g) + Br₂(g) → 2NOBr(g) The following reaction is at equilibrium in a closed 4L vessel: N₂(g) + 3H₂(g) ⇌ 2NH₃(g) What will happen if the vessel volume is reduced to 3L? (Assume constant temperature.) If Kc = 82 for the reaction below at 200 K, then what is the value of Kp? 2 NO₂ (g) ⇌ N₂O₄ (g) Consider the reaction: N₂ (g) + 3 Br₂ (g) ⇌ 2 NBr₃ (g) At equilibrium, the concentrations of N₂ and Br₂ are 0.34 M and 0.70 M respectively, and the concentration of NBr₃ is 0.090 M. What is Kc for this equilibrium?
10. The reaction 2NO+2H₂ →→→ N₂ + 2H₂O is proposed to occur through the following two elementary steps: k₂ H₂(g) + 2NO(g)- N₂O(g) + H₂O(g) H₂(g) + N₂O(g) N₂(g) + H₂O(g) By using the steady state approximation, what would be its rate expression? A) R = K[H₂][NO]2 B) R= K[H₂][NO] C) R = K1 K2 [H₂][NO]2 D) R=(k/k₂) [H₂][NO]2 E) R = K[H₂]2[NO]² *
The reaction 2 NO(g) + O2(g) --> 2 NO2(g) proceeds through the following mechanism: 2 NO(g) --> N2O2(g)N2O2(g) + O2(g) --> 2 NO2(g) (a) The second step of this mechanism is rate-determining (slow). What is the rate law for this reaction? Rate = k [NO] [O2] Rate = k [NO]2 [O2] Rate = k [NO] [O2]2 Rate = k [NO]1/2 [O2] Rate = k [NO] [O2]1/2 Rate = k [NO]2 Rate = k [NO]2 [O2]1/2 (b) What would the rate law be if the first step of this mechanism were rate-determining? Rate = k [NO] [O2] Rate = k [NO]2 [O2] Rate = k [NO] [O2]2 Rate = k [NO]1/2 [O2] Rate = k [NO] [O2]1/2 Rate = k [NO]2 Rate = k [NO]2 [O2]1/2 Rate = k [NO]
The following mechanism has been proposed for the conversion of ozone to oxygen in the gas phase. step 1 fast: O3 02 +0 step 2 slow: 03+0 →2 02 (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) Enter the formula of any species that acts as a reaction intermediate? If none leave box blank: (3) Complete the rate law for the overall reaction that is consistent with this mechanism. Use the form k[A]"[B]"... , where '1' is understood (so don't write it if it's a '1') for m, n etc. Rate =
The decomposition of N2O5 to NO2 and O2 is first order with respect to the reactant N2O5 and first order overall. The rate constant for the reaction at 70.oC is 6.82x10-3 s-1. The reaction is started with 0.300 mol of N2O5 in a 0.500L container. How many minutes will it take for the concentration of N2O5 to drop to 0.145M?
A proposed mechanism for the decomposition of hydrogen peroxide consists of three elementary steps: (1) H₂O2(g) →>> 2OH(g) (2) H₂O2(g) + OH(g) → H₂O(g) + HO₂(g) (3) HO₂(g) + OH(g) → H₂O(g) + O₂(g) If the rate law for the reaction is first order in H₂O2, which step in the mechanism is the rate-determining step? O Step 1 O None of the steps O Step 3 O Impossible to determine Steps 1 and 2 O All of the steps O Step 2 Hint: The slowest step in a mechanism determines the rate law. From each elementary reaction we can write a rate-law expression. Submit Question
Using the data in the table, determine the rate constant of the reaction and select the appropriate units. k = A + 2B → C + D Trial [A] (M) [B] (M) Rate (M/s) 1 0.260 0.260 2 0.260 0.520 3 0.520 0.260 Units 0.0199 0.0199 0.0796
Consider the overall reaction 2A + B ⇌ 2C(g) with proposed mechanism for this reaction: A + B ⇌ C + D (slow) A+D ⇌ C (fast)What is the rate law for this proposed mechanism?
What is the rate law for each of the following elementary reactions? (Use k for the rate constant.) 2NO2 = N2O4
Writing the rate law implied by a simple mechanism with an initial slow... Suppose the formation of nitryl fluoride proceeds by the following mechanism: elementary reaction step 1 NO₂ (g) +F₂ (g) 2 k₁ k₂ 2 F (g) + NO₂(g) → NO₂F (g) 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. NO₂F (g) +F (g) Note: your answer should not contain the concentrations of any intermediates. rate constant rate = k 0+ 00 X Ś
Suppose the reaction between nitric oxide and bromine proceeds by the following mechanism: step elementary reaction 1 NO (g) + Br₂ (g) → NOBr₂ (g) k₁ k₂ 2 NOBr₂ (g) + NO (g) → 2NOBr (g) 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. 0 rate = k rate constant 010 X Ś