6) For the reaction 3A + 2B2C + D + E, the initial reaction rate was measured for various initialconcentrations of reactants. The following data were collected:Rate (M/s)1.9 x 108[A] (M)[B] (M)1.0 x 10¹21.0 x 10¹19.5 x 1085.0 x 10¹21.0 x 101135.7 x 1081.0 x 10¹23.0 x 10¹1a) Write the rate law for this reaction.rate=[A]*[B]Y33.0 x 10" 1.0 x10¹2y = ²/5.0×101.0x1010X ==11.0x10"1.0 ×101053=1b) What is the overall order of the reaction?c) Calculate the rate law constant, k (including units).x==1.0x10"1.0 x 10"1lomC²

Answered: Image /qna-images/answer/e2d86c4a-e611-4e4c-a044-ca7e4eecf5aa.jpg

6) For the reaction 3A + 2B2C + D + E, the initial reaction rate was measured for various concentrations of reactants. The following data were collected: Rate (M/s) 1.9 x 108 [A] (M) [B] (M) 1.0 x 10¹2 1 1.0 x 1011 8 5.0 x 10¹2 9.5 x 108 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 X= = 1 1.0 x 10" 1.0×10 3 = 1 b) What is the overall order of the reaction? c) Calculate the rate law constant, k (including units). 5.0 x 10 1.0x101 5 = = lom 1.0×10" ex 1.0 x 10" 1 $62 or to 22squelon sitt stein

6) For the reaction 3A + 2B2C + D + E, the initial reaction rate was measured for various concentrations of reactants. The following data were collected: Rate (M/s) 1.9 x 108 [A] (M) [B] (M) 1.0 x 10¹2 1 1.0 x 1011 8 5.0 x 10¹2 9.5 x 108 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 X= = 1 1.0 x 10" 1.0×10 3 = 1 b) What is the overall order of the reaction? c) Calculate the rate law constant, k (including units). 5.0 x 10 1.0x101 5 = = lom 1.0×10" ex 1.0 x 10" 1 $62 or to 22squelon sitt stein

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 balanced equation for a given reaction is 4 X + 3 Y → P. The following data regarding initial reaction rates were collected in the lab. What is the rate law for the reaction? Trial [X] (M) [Y] (M) Rate (M/s) 1 0.020 0.060 3.40 x 10–3 2 0.020 0.120 2.72 x 10–2 3 0.080 0.060 1.36 x 10–2
Using the data in the table, calculate the rate constant of this reaction. k= A+B → C + D Trial [A] (M) [B] (M) 1 0.290 0.380 2 0.290 1.03 3 0.464 0.380 Units Rate (M/s) 0.0163 0.119 0.0261
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 hypothetical reaction: A + B + 2C → 2D + E where the rate law is Rate = -ALA) = k[A][B]2 An experiment is carried out where [Alo = 7.200 x 102 M, [B]. = 2.500 M and [Cla = 2.500 M. The reaction is started, and after 11.60 seconds, the concentration of A is 2.200 x 10° M. Calculate the value of k for this reaction in units of M2s1. Answer:
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
Using the information in the table, the value of the rate constant for the reaction A(g) + 3 B(g) → C(g) + 2 D(g) is Rate [A]. (M) [B]o (М) A) 0.106 M-'s-1 (M/s) В) 6.80 М-1s-1 1.25 0.100 0.850 C) 0.362 s-1 1.25 0.300 2.55 D) 68 M-3 s-1 E) 1.36 s-1 3.75 0.200 5.10
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
The concentration of A was monitored for the reaction A → P and the following data were obtained. What is the rate law, rate = k [A]x, for this reaction? [A] (M) Time (s) 0.0200 0 0.0169 100 0.0142 200 0.0120 300 0.0101 400 0.0086 500 0.0072 600 0.0061 700 Question 15 options: rate = 1.7 x 10–3 [A] rate = 2.3 x 10–3 [A]2 rate = 0 54 [A] rate = 1.3 x 10–3 [A] rate = 0 54 [A]2
The iodide ion reacts with hypochlorite ion (the active ingredient in chlorine bleaches) in the following way: OCII → OI¯ + Cl¯ This rapid reaction gives the following rate data: |[OCI¯] (M) [I¯] (M) Initial Rate (M/s) 1.36 × 10-4 1.5 × 10- -3 3.0 × 10-³ 1.5 x 10- -3 1.5 x 10 -3 1.5 × 10-³ 3.0 × 10-³ 2.72 × 10-4 2.72 × 10-4 Calculate the rate constant with proper units. Express the rate constant to two significant figures. Indicate the multiplication of units, as necessary, explicitly either with a multiplication dot or a dash (e.g. ft * lb or ft-lb). k Submit Part C HÅ Value Request Answer Units ? Calculate the rate when [OC] = 2.3 × 10-³ and [I¯] = 6.0 × 10-4 Express the rate in molarity per second to two significant figures.