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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