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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)

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    https://brainmass.com/chemistry/chemical-kinetics/rate-law-and-kinetics-115131

    Solution Preview

    Please see attached file.

    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.

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