The reaction 2 NO(8) + Cl2(8) → 2 NOCI(8) was per- formed and the following data were obtained under con- ditions of constant [Cl,]: (under conditions of constant [Cl2]) Time (a) Is the following mechanism consistent with the data? NO(8) + Cl2(8) = NOCI2(8) (fast) NOCI(8) + NO(8) → 2 NOCI(8) (slow) (b) Does the linear plot guarantee that the overall rate law is second order? (ONI/I

The reaction 2 NO(8) + Cl2(8) → 2 NOCI(8) was per- formed and the following data were obtained under con- ditions of constant [Cl,]: (under conditions of constant [Cl2]) Time (a) Is the following mechanism consistent with the data? NO(8) + Cl2(8) = NOCI2(8) (fast) NOCI(8) + NO(8) → 2 NOCI(8) (slow) (b) Does the linear plot guarantee that the overall rate law is second order? (ONI/I

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

The following mechanism has been suggested for the reaction: H:O: + 2H* + 21- l: + 2H:0 H:O2 +1-+ HOI + OH- Slow Fast OH-+H H:0 HOI + H +1-+1- H0 Fast Identify the rate law that is consistent with this mechanism. Multiple Choice Rate KHOIJOH) Rane - KH202H2 Rate - KHOITH"I Rate H202) Rate KCH TH")
Suppose the formation of tert-butanol proceeds by the following mechanism: step elementary reaction rate constant 1 CH33CBr (aq) → CH33C+ (aq) + Br− (aq) k1 2 CH33C+ (aq) + OH− (aq) → CH33COH (aq) k2 Suppose also k1 ≫ k2 . That is, the first step is much faster than the second.
What is the rate law for the following mechanism in terms of the overall rate constant k? Step 1:. A+B Step 2: B+C → D (slow) C (fast) Express your answer in terms of k and the necessary concentrations (e.g., k* [A] ^3*[D]). > View Available Hint(s) nV ΑΣφ 5E.. rate =
1(a) A reaction is observed to have the following rate constants at the indicated temperatures. Assuming the frequency factor remains the same, estimate the activation energy of the reaction. T (in °C) 20 40 k (in per second) 45 576 O - 97000 J mol1 O ~97 J mol 1 O ~847 J mol1 O - 8.47 J mol·1 O ~847000 J mol1 1(b) The density of air at STP is 1.285 g/L. Which of the following cannot be used to fill a balloon that will float in air at STP? O NO O NH3 O HE O Ne O CH4
The reaction 2 H2O2(aq) ➝ 2 H2O(l) + O2(g) is first order in H2O2 and under certain conditions has a rate constant of k = 0.00752 s-1 at 20.0ºC. A reaction vessel initially contains 150.0 mL of 30.0 % H2O2 by mass solution. The density of the solution is 1.11 g/mL. The gaseous oxygen is collected over water at 20.0ºC as it forms. What volume of O2 forms in 85.0 seconds at a barometric pressure of 742.5 mmHg? The vapor pressure of water at this temperature is 17.5 mmHg.
The gas phase decomposition of nitrogen dioxide at 383 °C NO₂(g) NO(g) + ½/0₂ (9) is second order in NO₂ with a rate constant of 0.540 M¹s¹. How much time is required for the concentration of NO₂ to drop to 4.85x10-2 M if its initial concentration is 0.385 M? S
The following mechanism for the gas phase decomposition of oxygen difluoride is consistent with the observed rate law. step 1 fast: 2 OF2=0;F4 step 2 slow: 0,F4¬0; +2 F; (1) What is the cquation 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 'I' is understood (so don't write it if it's a 'l') for m, n etc.
The recombination reaction2 HO2(g) → H2O2(g) + O2(g)has a second-order rate constant of 1.7E9 M-1 s-1. Calculate the half-life of the reaction if the initial concentration of HO2(g) is 2.22E-11 M.Note: the coefficient 2 in the reaction means that the integrated rate law for this reaction is:1/ct = 1/c0 + 2kt Give the answer to 3 significant figures
What is the rate law for the proposed mechanism? A) rate = k[H2][NO] H2(g) + 2NO(g) → N2O(g) + H2O(g) k[H•J°[NO] Step 1 (slow) B) rate = rate = k[H:][NO]? %3D N20(g) + H2(g) –→ N2(g) + H2O(g) Step 2 (fast) D) rate = k[H:]°[NO]? E) rate = k[H:][N:O]
The reaction described by H, (g) + L,(g) 2 HI(g) has an experimentally determined rate law of rate = k [H2] [I2] Some proposed mechanisms for this reaction are: Mechanism A k1 (1) H,(g) + L,(g) → 2 HI(g) (one-step reaction) Mechanism B k1 =2 I(g) k_1 (1) L(g) ; (fast, equilibrium) k2 (2) H, (g) + 2 I(g) 2 HI(g) (slow) Mechanism C k1 = 2 I(g) (fast, equilibrium) (1) k2 (2) I(g) + H, (g) HI(g) + H(g) (slow) (3) H(g) + I(g) → HI(g) (fast) Question Sourc
The reaction described by the following equation: 21-(aq) + H;O2(aq) + 2H*(aq) → I:(aq) + 2H;O(aq) has an experimental rate law (v) = k[I][H2O2]. Suggest a plausible mechanism for this reaction, and identify the rate-determining step.
The gas-phase reaction 2NO2Br →2NO2 + Br2 has r = k[NO2Br]. Devise a mechanism consistent with this rate law.