Answered: If you have a reaction A + B --> C, and…

If you have a reaction A + B --> C, and the rate equation is Rate = k [A], what can you infer about the mechanism of the reaction?

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 data in the table below were obtained for the reaction: A + B → PRODUCT Experiment Number [A] (M) |[B] (M)| (M/s) |Initial Rate 1 0.273 0.763 2.83 0.273 1.526 2.83 0.819 0.763 25.47 The rate law for this reaction is rate =
Consider the following reaction: 4 HBr(g) + O2(g) 2 H2O(g) + 2 Br2(g)(a) The rate law for this reaction is first order in HBr(g) and first order in O2(g). What is the rate law for this reaction?(b) If the rate constant for this reaction at a certain temperature is 8.80e+03, what is the reaction rate when [HBr(g)] = 0.00429 M and [O2(g)] = 0.00758 M?Rate = _______ M/s.(c) What is the reaction rate when the concentration of HBr(g) is doubled, to 0.00858 M while the concentration of O2(g) is 0.00758 M?Rate = _______ M/s
Consider the reaction and its rate law. 3A+3B⟶productsrate=?[A][B]2 What is the order with respect to A?
The rate law for the reaction 2A → B is second order in A. The following figure represents samples with different concentrations of A; the red spheres represent molecules of A. In which sample will the reaction proceed most rapidly?
6) For the reaction 3A + 2B2C + D + E, the initial reaction rate was measured for various initial concentrations of reactants. The following data were collected: Rate (M/s) 1.9 x 108 [A] (M) [B] (M) 1.0 x 10¹2 1.0 x 10¹1 9.5 x 108 5.0 x 10¹2 1.0 x 1011 3 5.7 x 108 1.0 x 10¹2 3.0 x 10¹1 a) Write the rate law for this reaction. rate=[A]*[B]Y 3 3.0 x 10" 1.0 x10¹2 y = ²/ 5.0×10 1.0x1010 X = = 1 1.0x10" 1.0 ×1010 5 3=1 b) What is the overall order of the reaction? c) Calculate the rate law constant, k (including units). x = = 1.0x10" 1.0 x 10" 1 lom C²
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
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
You are studying the reaction A₂(g)+B₂(g) →2AB(g) to determine its rate law. Assuming that you have a valid exper-imental procedure for obtaining [A₂] and [B₂] at various times,explain how you determine (a) the initial rate, (b) the reaction orders, and (c) the rate constant.
You and your lab partner are studying the rate of a reaction, A + B --> C. You make measurements of the initial rate under the following conditions: (b) For a reaction of the form, A + B + C --> reaction from the choices below. (a) Which of the following reactant concentrations could you use for experiment 3 in order to determine the rate law, assuming that the rate law is of the form, Rate = k [A] [B]Y? Choose all correct possibilities. O [A] = 0.2 and [B] = 1.0 O [A] = 0.4 and [B] = 1.0 O [A] = 0.8 and [B] = 0.5 O [A] = 0.6 and [B] = 0.5 O [A] = 0.2 and [B] = 1.5 O [A] = 0.4 and [B] = 0.5 O [A] = 0.4 and [B] = 1.5 O [A] = 1.0 and [B] = 0.5 O Rate = K[A][B][C] O Rate = K[A][C] O Rate = K[A]²[C] T O Rate = k[A][C]² O Rate = K[A]²[C]² O Rate = K[A]³ [c] O Rate = K[A][C]³ the following Experiment [A] (M) [B] (M) Rate (M/s) 0.5 0.5 The rate will be the original rate multiplied by a factor of 0.2 0.4 (c) By what factor will the rate of the reaction described in part (b) above change if the…
What is the effective rate constant [in units that combine M and min] for the reaction with rate law v = k[A][B]2 where k = 0.54 M -2 min-1 if the initial concentration of B is 3.7 molar and that of A is 0.032 molar?
Given the following data, determine the rate constant of the reaction 2NO(g) + Cl2(g) –→ 2NOCI(g) Experiment [NO] (M) |Ck] (M) Rate (M/s) 0.0300 0.0100 3.4 x 104 0.0150 0.0100 8.5 x 10-5 3 0.0150 0.0400 3.4 x 104
Hydrogen peroxide decomposes spontaneously to yield water and oxygen gas according to the reaction equation 2H,0, (aq) — 2н,00) + 0,(8) The activation energy for this reaction is 75 kJ-mol-1. In the presence of a metal catalyst, the activation energy is lowered to 49 kJ-mol-1. At what temperature would the non-catalyzed reaction need to be run to have a rate equal to that of the metal-catalyzed reaction at 25 °C? T = K