O KINETICS AND EQUILIBRIUM Writing the rate law implied by a simple mechanism Suppose the reaction between nitric oxide and bromine proceeds by the following mechanism: step elementary reaction rate constant 1 NO(g) + Br,(g) → NOB1,(g) NOBr, (g) + N0(g) →2 NOB1(g) Suppose also k,»k,. That is, the first step is much faster than the second. Write the balanced On 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 k = the reverse of the two elementary reactions in the mechanism. olo

O KINETICS AND EQUILIBRIUM Writing the rate law implied by a simple mechanism Suppose the reaction between nitric oxide and bromine proceeds by the following mechanism: step elementary reaction rate constant 1 NO(g) + Br,(g) → NOB1,(g) NOBr, (g) + N0(g) →2 NOB1(g) Suppose also k,»k,. That is, the first step is much faster than the second. Write the balanced On 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 k = the reverse of the two elementary reactions in the mechanism. olo

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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(4) Use the following experimental data to write the rate law and the rate constant for the reaction 2 NO (g) + O2 (g) = 2 NO2 (g) Experiment [NO] (M) [O2] (M) Initial rate (M/s) 1 0.0100 0.0100 0.711 x 10-2 2 0.0100 0.0400 2.84 x 10-2 3 0.0200 0.0100 2.84 x 10-2
The rate equation for the hydrolysis of sucrose to fructose and glucose C12 H22 O11 (aq) + H₂O(l) → C6H12O6 (aq) + C6H12O6 (aq) is -A[sucrose]/At = k[C12H22 O11]. After 21 minutes at 27 °C, the sucrose concentration decreased from 0.0139 M to 0.0129 M. Find the rate constant k. k = min-1
Question 17 of 19 Submit What is the rate law for the proposed mechanism? A) rate = k[H2][NO] H2(g) + 2NO(g) → N20(g) + H2O(g) B) rate = k[Hzl°[NO] Step 1 (slow) C) rate = k[H2][NO]? N20(g) + H2(g) N2(g) + H2O(g) Step 2 (fast) D) rate = k[H2l°[NO]? E) rate = k[H2][N2O]
1
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 formation of nitrosyl chloride is described by the following chemical equation: 2NO (g) + Cl₂ (g) → 2NOCI (g) Suppose a two-step mechanism is proposed for this reaction, beginning with this elementary reaction: NO (g) +Cl₂ (g) NOCI₂ (g) Suppose also that the second step of the mechanism should be bimolecular. Suggest a reasonable second step. That is, write the balanced chemical equation of a bimolecular elementary reaction that would complete the proposed mechanism. 11 × Ś
= ○ KINETICS AND EQUILIBRIUM Expressing the concentration of an intermediate in terms of the... Consider the following elementary reaction: CFC1₂(g) → CFC1₂(g) +C1(g) Suppose we let k₁ stand for the rate constant of this reaction, and k_₁ stand for the rate constant of the reverse reaction. 1 Write an expression that gives the equilibrium concentration of CFC1, in terms of k₁, k₁, and the equilibrium concentrations of CFC13 and C1. 1' [CFC₁₂] = 0 √6 X 5 0/5
Consider the following reaction: 2N₂O(g) → 2N2(g) + O2(g) Part A Express the rate of the reaction in terms of the change in concentration of each of the reactants and products. Rate = 1 A[₂0] At O Rate = O Rate - Submit Rate = -A[₂0] At Correct Part B Rate = Submit A[N₂O] At Part C A[N₂0] At A[N₂O] At Previous Answers Submit Request Answer 1 A[N₂] 2 At At In the first 13.0 s of the reaction, 1.9x10-2 mol of O₂ is produced in a reaction vessel with a volume of 0.280 L. What is the average rate of the reaction over this time interval? Express your answer using two significant figures. IVE| ΑΣΦ Request Answer A[N₂] At 1 A[N₂] At 1/1 A[0₂] At A[0₂] At A[0₂] A[0₂] At Predict the rate of change in the concentration of N₂O over this time interval. In other words, what is A[N₂O]/At? Express your answer using two significant figures. IVE| ΑΣΦ ? M-s-1 ? M-s-1
Derive the unit for K then using K at 904 degrees celsius, find the rate of reaction at the instant when [NO]=0.470 M and [H2] = 0.315M
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Consider the mechanism. Step 1: Step 2: Overall: A B+C C+D E - equilibrium slow A+DB+E Determine the rate law for the overall reaction, where the overall rate constant is represented as k.
2. At 325°C, N0,(g) reacts with CO(g) to yield NO(g) and CO,(g). The reaction is: NO,(g) + CO(g) I NO(g) + CO,(g) It is observed that the reaction rate does not depend upon the concentration of CO, and t\so the reaction rate law does not involve [CO]. The rate does depend upon [NO,], however, and the following data is obtained. Determine the rate law and the value of the rate constant. Rate ( M sec ') NO,] 1. 1 X 10 -2 0.15 4.5 X 10-2 0.3 1.8 X 10- 4.0 X 10-13 0.6 0.9