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  # rate law and kinetics
  
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  1.) At 40 degrees Celsius CH2O2(aq) will decompose according to the following reaction:
  2H2O2(aq) ----- 2H2O(l) + O2(g)
  The following data were collected for the concentration of H2O2 at various times.
  Times(s) [H2O2](M)
  0 1.000
  2.16x10^4 0.500
  4.32x10^4 0.250
  a.) Calculate the average rate of decomposition of H2O2 between 0 and 2.16x10^4 s. Use this rate to calculate the rate of production of O2(g).
  b.) What are these rates for the time period 2.16x10^4 s to 4.32x10^4 s?
  
  2.) Use the given data for the hypothetical reaction:
  2A + B ----- products
  to determine the rate law and to evaluate the rate constant at 30 degrees Celsius.
  Reaction # [A] [B] Initial rate (mol/L s)
  1 0.1 0.1 3x10^(-2)
  2 0.1 0.3 3x10^(-2)
  3 0.2 0.3 6x10^(-2)
  
  3.) Derive the rate law expression and calculate the rate constant for the reaction:
  A + B + 3C ----- products
  given the following data for 15 degrees Celsius.
  Reaction # [A] [B] [C] Initial rate (mol/L s)
  1 0.4 0.1 0.1 6.0x10^(-3)
  2 0.4 0.2 0.1 6.0x10^(-3)
  3 0.4 0.3 0.2 1.2x10^(-2)
  4 1.2 0.4 0.2 0.11
  
  4.) Indicate the overall order of reaction for each of the following rate laws.
  a.) R=k[NO2][F2]
  b.) R=k[I]^2[H2]
  c.) R=k[H2][Cl2]^(1/2)
  
  https://brainmass.com/chemistry/chemical-kinetics/rate-law-and-kinetics-115131
  
  #### Solution Preview
  
  1.) At 40 degrees Celsius CH2O2(aq) will decompose according to the following reaction:
  2H2O2(aq) ----- 2H2O(l) + O2(g)
  The following data were collected for the concentration of H2O2 at various times.
  Times(s) [H2O2](M)
  0 1.000
  2.16x10^4 0.500
  4.32x10^4 0.250
  a.) Calculate the average rate of decomposition of H2O2 between 0 and 2.16x10^4 s. Use this rate to calculate the rate of production of O2(g).
  
  rate = -1/2 d[H2O2]/dT = d[O2]/dT
  
  so, d[O2]/dT = -1/2 (1.000 - 0.500)/ (0 - 2.16x10^4)
  = 1.157 x 10^-5 Ms-1
  
  b.) What are these rates for the time period 2.16x10^4 s to 4.32x10^4 s?
  
  d[O2]/dT = -1/2 (0.500 - 0.250)/ (2.16x10^4 -4.32x10^4 )
  = 5.787 x 10^-6 Ms-1
  
  2.) Use the given data for the ...
  
  #### Solution Summary
  
  Rate law and kinetics of the reactions are investigated.
  
  \$2.49
explanation: The document contains multiple chemistry questions related to chemical kinetics and rate laws. Each question involves calculations or derivations to determine reaction rates, rate laws, and rate constants based on given data. The questions are not accompanied by answers, only the problems are presented.
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distilabel_metadata.role: system
distilabel_metadata.content: Explore BrainMass
  
  # rate law and kinetics
  
  Not what you're looking for? Search our solutions OR ask your own Custom question.
  
  This content was COPIED from BrainMass.com - View the original, and get the already-completed solution here!
  
  1.) At 40 degrees Celsius CH2O2(aq) will decompose according to the following reaction:
  2H2O2(aq) ----- 2H2O(l) + O2(g)
  The following data were collected for the concentration of H2O2 at various times.
  Times(s) [H2O2](M)
  0 1.000
  2.16x10^4 0.500
  4.32x10^4 0.250
  a.) Calculate the average rate of decomposition of H2O2 between 0 and 2.16x10^4 s. Use this rate to calculate the rate of production of O2(g).
  b.) What are these rates for the time period 2.16x10^4 s to 4.32x10^4 s?
  
  2.) Use the given data for the hypothetical reaction:
  2A + B ----- products
  to determine the rate law and to evaluate the rate constant at 30 degrees Celsius.
  Reaction # [A] [B] Initial rate (mol/L s)
  1 0.1 0.1 3x10^(-2)
  2 0.1 0.3 3x10^(-2)
  3 0.2 0.3 6x10^(-2)
  
  3.) Derive the rate law expression and calculate the rate constant for the reaction:
  A + B + 3C ----- products
  given the following data for 15 degrees Celsius.
  Reaction # [A] [B] [C] Initial rate (mol/L s)
  1 0.4 0.1 0.1 6.0x10^(-3)
  2 0.4 0.2 0.1 6.0x10^(-3)
  3 0.4 0.3 0.2 1.2x10^(-2)
  4 1.2 0.4 0.2 0.11
  
  4.) Indicate the overall order of reaction for each of the following rate laws.
  a.) R=k[NO2][F2]
  b.) R=k[I]^2[H2]
  c.) R=k[H2][Cl2]^(1/2)
  
  https://brainmass.com/chemistry/chemical-kinetics/rate-law-and-kinetics-115131
  
  #### Solution Preview
  
  1.) At 40 degrees Celsius CH2O2(aq) will decompose according to the following reaction:
  2H2O2(aq) ----- 2H2O(l) + O2(g)
  The following data were collected for the concentration of H2O2 at various times.
  Times(s) [H2O2](M)
  0 1.000
  2.16x10^4 0.500
  4.32x10^4 0.250
  a.) Calculate the average rate of decomposition of H2O2 between 0 and 2.16x10^4 s. Use this rate to calculate the rate of production of O2(g).
  
  rate = -1/2 d[H2O2]/dT = d[O2]/dT
  
  so, d[O2]/dT = -1/2 (1.000 - 0.500)/ (0 - 2.16x10^4)
  = 1.157 x 10^-5 Ms-1
  
  b.) What are these rates for the time period 2.16x10^4 s to 4.32x10^4 s?
  
  d[O2]/dT = -1/2 (0.500 - 0.250)/ (2.16x10^4 -4.32x10^4 )
  = 5.787 x 10^-6 Ms-1
  
  2.) Use the given data for the ...
  
  #### Solution Summary
  
  Rate law and kinetics of the reactions are investigated.
  
  \$2.49
distilabel_metadata.role: user
distilabel_metadata.raw_output_q_a_detector_0: The document contains multiple chemistry questions related to chemical kinetics and rate laws. Each question involves calculations or derivations to determine reaction rates, rate laws, and rate constants based on given data. The questions are not accompanied by answers, only the problems are presented.
  
  Label: multiple-question