Problems requiring More Work 1. The decomposition of hydrogen peroxide was studied and the data below was collected and graphed as shown in the 3 graphs. 2 H2O2 (I) → 2 H2O (I) + 02(g) time, s [H,O,1,mol/L In[H;O] 1/[H;O;] 25 y = 0.004596x - 0.847 R = 0.872 1 20 120 0.91 -0.09431 1.098901 15 300 0.78 -0,24846 1.282051 600 0.59 -0.52763 1.694915 10 1200 0.37 -0.99425 2.702703 1800 0.22 -1.51413 4.545455 2400 0.13 -2.04022 7.692308 1000 2000 3000 4000 3000 0.082 -2.50104 12.19512 -5 time, s 3600 0.05 -2.99573 20 1.5 .1000 2000 3000 4000 y=-0.000264x+0.841 R2 = 0,889 1 -1 0.5 -2 y = -0.000835x - 0.00493 R = 0.99978 %3D 1000 2000 3000 4000 -0.5 -4 time, s time, s a. Write the general form of the rate law for the decomposition of hydrogen peroxide with respect to the disappearance of the hydrogen peroxide. b. What is the order of reaction with respect to [H2O2]? How did you determine this? c. Write the integrated rate law, including the value of the rate constant with units. d. Calculate the concentration of H2O2 after the reaction has run for 45.0 minutes. (Use the integrated rate law from c and show your work.) e. Calculate the half life of this reaction [H,O;] , M 1/[H,O,] , M-1

Problems requiring More Work 1. The decomposition of hydrogen peroxide was studied and the data below was collected and graphed as shown in the 3 graphs. 2 H2O2 (I) → 2 H2O (I) + 02(g) time, s [H,O,1,mol/L In[H;O] 1/[H;O;] 25 y = 0.004596x - 0.847 R = 0.872 1 20 120 0.91 -0.09431 1.098901 15 300 0.78 -0,24846 1.282051 600 0.59 -0.52763 1.694915 10 1200 0.37 -0.99425 2.702703 1800 0.22 -1.51413 4.545455 2400 0.13 -2.04022 7.692308 1000 2000 3000 4000 3000 0.082 -2.50104 12.19512 -5 time, s 3600 0.05 -2.99573 20 1.5 .1000 2000 3000 4000 y=-0.000264x+0.841 R2 = 0,889 1 -1 0.5 -2 y = -0.000835x - 0.00493 R = 0.99978 %3D 1000 2000 3000 4000 -0.5 -4 time, s time, s a. Write the general form of the rate law for the decomposition of hydrogen peroxide with respect to the disappearance of the hydrogen peroxide. b. What is the order of reaction with respect to [H2O2]? How did you determine this? c. Write the integrated rate law, including the value of the rate constant with units. d. Calculate the concentration of H2O2 after the reaction has run for 45.0 minutes. (Use the integrated rate law from c and show your work.) e. Calculate the half life of this reaction [H,O;] , M 1/[H,O,] , M-1

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 58E: Consider the hypothetical reaction A+B+2C2D+3E where the rate law is Rate=[A]t=k[A][B]2 An...

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