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
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Enter your answer in the provided box. Consider the reaction: 2NO(g) + 0,(g) → 2NO2(g) Suppose that a particular moment during the reaction nitric oxide (NO) is reacting at a rate of 0.068 Mis. At what rate is molecular oxygen reacting? M Molecular oxygen is (select) (select) |at a rate of consumed produced
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]
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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
74.) Refer to the following reaction mechanism 2A - B ki B 2A k.1 B + C → D k2 Luse the pre-equilibrium method to determine the rate law of the reaction. ause the steady state approximation assuming that the first step is the slowest step. aluse the steady state approximation assuming that the third step is the slowest step.
= ○ 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
In a reaction where A and B go to products, what is the rate law if the following rates are observed? [B] mol/L [A] mol/L 0.020 rate M/s 0.010 0.278 0.040 0.010 0.556 0.030 0.020 1.67 0.040 0.020 2.22 A rate - kIA) (B}? B) rate = k[A][B] rate = k[A][B]? O rate = k[AJ [B]