The image contains three graphs analyzing the decomposition of compound B. Each graph plots concentration data over time to determine the reaction order and rate constant.1. **Graph [B] vs. time:** - The y-axis represents the concentration of compound B in molarity (M). - The x-axis represents time in minutes. - The plotted data points form a downward sloping line. - The linear regression equation is \( y = -6E-05x + 0.0093 \) with \( R^2 = 0.9498 \).2. **Graph ln[B] vs. time:** - The y-axis represents the natural logarithm of the concentration of compound B. - The x-axis represents time in minutes. - The plotted data points form a downward sloping line. - The linear regression equation is \( y = -0.0078x - 4.6522 \) with \( R^2 = 0.9872 \).3. **Graph 1/[B] vs. time:** - The y-axis represents the inverse concentration of compound B (1/M). - The x-axis represents time in minutes. - The plotted data points form an upward sloping line. - The linear regression equation is \( y = 1.3333x + 100 \) with \( R^2 = 1 \).**Analysis:**- The graph of 1/[B] vs. time shows a perfect linear relationship with an \( R^2 \) value of 1, indicating that the decomposition follows second-order kinetics.- The rate constant (\( k \)) can be determined from the slope of the line in the 1/[B] vs. time graph: \( k = 1.3333 \) M\(^{-1}\)min\(^{-1}\).

The information below is for the decomposition of compound B. What is the rate law for this decomposition, and what is the rate constant? [B] (M) 1/[B] (1/M) 0.0111 0.0101 0.0091 0.0081 0.0071 0.0061 0.0051 0.0041 240 220 200 180 8 140 120 100 I 0 0 10 10 20 20 30 30 [B] vs time 40 40 50 time (min) 1/[B] vs time 50 time (min) 60 60 y=-6E-05x+0.0093 R2=0.9494 70 80 y=1.3333x+100 R²=1 70 90 100 80 90 100 In [B] -4.61 -4.7 -4.8 -4.9 -5 -5.1 -5.2 -5.3 -5.4 -5.5 Q 10 20 30 In [B] vs time 40 50 time (min) 60 70 80 y=-0.0087x-4.6522 R²=0.9872 90 100

The information below is for the decomposition of compound B. What is the rate law for this decomposition, and what is the rate constant? [B] (M) 1/[B] (1/M) 0.0111 0.0101 0.0091 0.0081 0.0071 0.0061 0.0051 0.0041 240 220 200 180 8 140 120 100 I 0 0 10 10 20 20 30 30 [B] vs time 40 40 50 time (min) 1/[B] vs time 50 time (min) 60 60 y=-6E-05x+0.0093 R2=0.9494 70 80 y=1.3333x+100 R²=1 70 90 100 80 90 100 In [B] -4.61 -4.7 -4.8 -4.9 -5 -5.1 -5.2 -5.3 -5.4 -5.5 Q 10 20 30 In [B] vs time 40 50 time (min) 60 70 80 y=-0.0087x-4.6522 R²=0.9872 90 100

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

Consider this reaction: 2C1₂05 (g) → 2Cl₂ (g) +50₂ (g) At a certain temperature it obeys this rate law. rate =(0.0913 s¯¹)[C₁₂05] Suppose a vessel contains Cl₂05 at a concentration of 0.460M. Calculate the concentration of C1₂O5 in the vessel 9.70 seconds later. You may assume no other reaction is important. 25 2 Round your answer to 2 significant digits. [ M x10
A reaction has a rate law of Rate = (1.25 M⁻²s⁻¹)[A][B]². What concentration of [B] would give the reaction a rate of 0.0355 M⁻¹s⁻¹ if the concentration of [A] is 0.250 M?
Using the data in the table, calculate the rate constant of Trial [A] (M) [B] (M) Rate (M/s) this reaction. 1. 0.400 0.210 0.0120 A +B C+D 2 0.400 0.525 0.0750 3 0.480 0.210 0.0144 Units k =
Using the data in the table, determine the rate constant of the Trial [A] (M) | [B] (M) Rate (M/s) reaction and select the appropriate units. 1 0.220 0.260 0.0189 2 0.220 0.520 0.0189 А + 2B → C+ D 3 0.440 0.260 0.0756 Units 0.0484 k M-'s-1 Incorrect
A2 -> 2A (slow) 2A + B2 -> 2AB (fast) What is the rate law for the overall reaction?
The following initial rate data are for the reaction of ICl with hydrogen:2 ICl + H2I2 + 2 HCl Experiment [ICl]o, M [H2]o, M Initial Rate, M s-1 1 0.438 0.105 9.37×10-3 2 0.876 0.105 1.87×10-2 3 0.438 0.209 3.71×10-2 4 0.876 0.209 7.42×10-2 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]n , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = _______ From these data, the rate constant is __________M-2s-1.
A valid mechanism for the following overall reaction is given below. Overall reaction: 2 NO (g) + Cl2 (g) → 2 NOCI (g) Step 1: NO (g) + Cl2 (g) → NOCI2 (g) Step 2: NOC12 (g) + NO (g) → 2 NOCI (g) (slow) (fast) What is the rate law for this reaction? Rate = k[NO]?[Cl2] Rate = k[NO][CI] Rate = k[NO][Cl2][NOCI] Rate = k[Cl2][NOC12]
or a reaction involving two reagents A and B, the following data was collected over three experiments. Exp# [A] [B] Rate (M/s) 1 0.20 M 0.20 M 5.0 2 0.20 M 0.40 M 20.0 3 0.10 M 0.40 M 10.0 Using the above data, which of the following is the rate law for the reaction of A with B?
Deducing a rate law from the change in concentration over time A chemistry graduate student is studying the rate of this reaction: 2HI (g) - H, (g) +L, (g) He fills a reaction vessel with HI and measures its concentration as the reaction proceeds: time [HI] (milliseconds) 0.100 M 10. 0.0494 M 20. 0.0328 M 30. 0.0245 M 40. 0.0196 M Use this data to answer the following questions. Write the rate law for this reaction. rate = k I Calculate the value of the rate constant k. k = Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol.
The following initial rate data are for the reaction of ICI with hydrogen: 2IC1 + H₂ → I₂ + 2HCl Experiment [IC]o, M [H₂], M 0.198 0.141 0.396 0.141 0.198 0.281 0.396 0.281 1 2 3 4 Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = k = -2 M-². Initial Rate, M. s-¹ S 0.00657 0.0131 0.0261 0.0522 -1 S
The information below is for the decomposition of compound D. What is the rate law for this decomposition, and what is the rate constant? @ 1/[D] 0.0034 0.0032 0.003 0.0028 0.0026 0.0024 0.0022 0.002 500 480 460 440 420 400 380 360 340 320 300 0 0 20 20 40 40 [D] vs t 60 60 t (min) 1/[D] vs t t (min) y=-1E-05x + 0.0032 R² = 0.9817 80 80 100 y = 1.5x + 300 R² = 1 O 100 O 120 120 140 140 -5.6 -5.7 -5.8 -5.9 In [D] -6 -6.1 -6.2 -6.3 0 20 40 In [D] vs time 60 80 t (min) 100 y = -0.0039x - 5.72 R2=0.9954 120 140