QUESTION 17 The rate law for reaction 2 A+B 2 C is experimentally determined to be first-order in [A] and first-order in B. Which of the following is consistent with the observed rate law? A → D B+D → E A+E→ 2C A+B →D A+D 2C OA OB. OC OD. OE. A+B D A+D → 2C 2A D B+D → E E-2C 2A+B →2C slow fast fast slow fast equilibrium fast equilibrium slow fast equilibrium slow fast slow 530 kJ/mol? Enter the

QUESTION 17 The rate law for reaction 2 A+B 2 C is experimentally determined to be first-order in [A] and first-order in B. Which of the following is consistent with the observed rate law? A → D B+D → E A+E→ 2C A+B →D A+D 2C OA OB. OC OD. OE. A+B D A+D → 2C 2A D B+D → E E-2C 2A+B →2C slow fast fast slow fast equilibrium fast equilibrium slow fast equilibrium slow fast slow 530 kJ/mol? Enter the

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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Compounds A and B react to form C and D in a reaction that is found to be second-order overall and second-order in B. The rate constant at 30°C is 0.622 liter per mole per minute. A+B→C+ D How many minutes does it take 4.0 x 10 2 MB (mixed with excess A) to be reduced to 3.3 x 10 -2 M B? O a. 6.4 min O b.5.0 min Oc.3.6 min O d. 1.4 min O e. 8.5 min
The data in the table below were obtained for the reaction: 2A+ 2B → 3C Experiment Number [A] (M) [В] (M) Initial Rate (M/s) 1 0.186 0.451 2.26 0.930 0.451 11.3 0.186 1.35 20.34 The rate law for this reaction is rate = O A. k[A]2 O B. k[A]²[B]2 O. k[A][B] O D. K[A][B]? O E. k[A]²[B]
Based on the observed rates in the experiments below, what is the rate law for the reaction 3A + 2B + C → G? Expt. # 1 2 3 4 Vo = K[A]²[B][C] Vo = K[A]²[B][C]-1 Vo = K[A]²[B]-¹[C] Vo = K[A][B]²[C] [A] (M) 0.20 0.10 0.10 0.30 [B] (M) 0.10 0.20 0.10 0.10 [C] (M) 0.10 0.20 0.20 0.10 vo (M/s) 0.20 0.050 0.10 0.45
At a particular temperature, N 20 5 decomposes according to a first-order rate law with a half-life of 3.0 s. If the initial concentration ofN 20 5 is 1.0 х 10 16 molecules/cm what will be the concentration in molecules/cm 3 after 11.5 s? O a. 1.0 × 1016 O b.2.3 × 10-1 O. 7.0× 1014 O d. 3.4 x 101 O e. 2,0 × 1014
Evaluate the following data to determine whether the reaction is first or second order. Calculate the rate constant and be certain to give its unit. A → Product A (mmol/L) Time (sec) 1.00 0 0.50 11 0.25 20 0.10 48 0.05 105
It was found that for the reaction 2 A + B → 3 C the rate law is Rate = k[A][B] · %3D At the initial concentrations [A]o = 0.100 M and [B]o = 0.200 M the initial rate is 0.0500 M/s. %3D What would be the initial rate if the initial concentrations were [A]o = 0.500 M and [B]o = 0.0750 M? 0.0352 M/s 0.0937 M/s O 0.0711 M/s 0.00533 M/s O 0.469 M/s
The reaction A + 2B → products has been found to have the rate law, rate = k[A] [B]2. While holding the concentration of A constant, the concentration of B is increased from x to 3x. By what factor does the rate of reaction increase? 3 fold 6 fold 9 fold 27 fold the rate of reaction does not change with a change in the [B].
The data in the table below were obtained for the reaction: 2A + 2B — зс Experiment Number [A] (M) [B] (M) Initial Rate (M/s) 1 0.775 0.321 0.082 2 1.51 0.321 0.082 3 0.775 0.963 0.738 The rate law for this reaction is rate = O A. k[A][B]² B. k[B]2 c. k[A][B] O D. K[A]2{B] O E. K[A]²[B]2
QUESTION 9 The reaction 2A(aq) + B(aq) → C(aq) + 3D(aq) is first order with respect to reactant A and second order with respect to B. At a certain temperature, when the concentration of A is 0.516 M and the concentration of B is 0.251 M, the initial reaction rate is 3.00 x 10-5 M/s. Calculate the rate constant for the reaction. Express your answer in scientific notation to 3 significant figures, INCLUDE units e.g. M-1s-1 or Ms-1 (no + sign, no spaces). If you do not follow these instructions, you will not get credit.
The integrated rate laws for zero-, first-, and second-order reaction may be arranged such that they resemble the equation for a straight line, y=mx+b. Order Integrated Rate Law Graph Slope 0 [A]=−kt+[A]0 [A] vs. t −k 1 ln[A]=−kt+ln[A]0 ln[A] vs. t −k 2 1[A]= kt+1[A]0 1[A] vs. t k The reactant concentration in a first-order reaction was 5.50×10−2 M after 25.0 s and 1.30×10−3 M after 100 s . What is the rate constant for this reaction? The reactant concentration in a second-order reaction was 0.250 M after 260 s and 6.60×10−2 M after 845 s . What is the rate constant for this reaction?
The expression, rate = k[A][B]2, would suggest which of the following steps to be the rate determining step in the overall reaction? step 1 A + B → C step 2 C + B → D + E step 3 D + A → products overall: 2A + 2B → products A. step1 B. step2 C. step3 D. overall reaction
Data for the reaction A + B → C are given below. Find the rate constant for this system. Experiment [A], M [B], M Initial rate, M/s 1 0.030 0.060 2.5 × 10-5 2 0.030 0.020 2.5 × 10-5 3 0.060 0.060 10.0 × 10-5 1.7 × 10-3 M-1s-1 2.8 × 10-2 M2s-1 1.7 × 10-3 Ms-1 2.8 × 10-2 M-1s-1 2.8 × 10-2 Ms-1