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Integrated Rate Law

#### Q. The acid-catalyzed decomposition of hydrogen peroxide is a first order reaction. An experiment is run (at 66°C) in which the initial concentration of hydrogen peroxide is 0.110 M. After 254 minutes the concentration of H2O2 remaining is 0.035 M. Overall reaction: 2H2O2 (aq) - > 2H2O (l) + O2 (g) b. what is the half-life at this temperature?

Solved • Mar 22, 2020

Integrated Rate Law

#### Q. The acid-catalyzed decomposition of hydrogen peroxide is a first order reaction. An experiment is run (at 66°C) in which the initial concentration of hydrogen peroxide is 0.110 M. After 254 minutes the concentration of H2O2 remaining is 0.035 M. Overall reaction: 2H2O2 (aq) - > 2H2O (l) + O2 (g) a. What is the value of the rate constant for this reaction at 66 degrees Celsius?

Solved • Mar 22, 2020

Integrated Rate Law

#### Q. a. How long will it take for 38.5% of nitrogen dioxide to decompose? b. What is the half-life of the reaction if initial concentration of nitrogen dioxide is 0.500 M.

Solved • Mar 22, 2020

Integrated Rate Law

#### Q. K1.The first order decomposition of C2H5Cl has a rate constant of 0.0128 min-1 at 425oC. If the initial concentration of the C2H5Cl is 0.35 M, calculate a. The concentration of the C2H5Cl after 15 minutes b. The half life for the reaction c. How long it will take for 80% of the original sample to decompose d. If the rate constant for the same reaction is 0.0170 min-1 at 470oC is what is the energy of activation for the reaction? e. Determine the rate constant at a temperature of 100oC.

Solved • Mar 22, 2020

Integrated Rate Law

#### Q. Explain at three ways that you can distinguish between zero order and first order reactions?

Solved • Mar 22, 2020

Integrated Rate Law

#### Q. The following data are obtained for the decomposition of CH3NO2 at 500K: Time (seconds) 0 300 600 900 1200 Concentration 0.200 0.145 0.105 0.076 0.055 a. Using this data, prepare separate graphs of Concentration vs. time, LN of concentration vs. time, and 1/Concentration vs. time to determine the order for the reaction. Explain why you selected this order. b. Determine the specific rate constant for the reaction and the half-life

Solved • Mar 20, 2020