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) At 40 degrees Celsius CH2O2(aq) will decompose according to the following reaction:

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)

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