# rate law and kinetics

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
2.16×10^4 0.500
4.32×10^4 0.250
a.) Calculate the average rate of decomposition of H2O2 between 0 and 2.16×10^4 s. Use this rate to calculate the rate of production of O2(g).
b.) What are these rates for the time period 2.16×10^4 s to 4.32×10^4 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 3×10^(-2)
2 0.1 0.3 3×10^(-2)
3 0.2 0.3 6×10^(-2)

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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 6.0×10^(-3)
2 0.4 0.2 0.1 6.0×10^(-3)
3 0.4 0.3 0.2 1.2×10^(-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)

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
2.16×10^4 0.500
4.32×10^4 0.250
a.) Calculate the average rate of decomposition of H2O2 between 0 and 2.16×10^4 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 – 2.16×10^4)
= 1.157 x 10^-5 Ms-1

b.) What are these rates for the time period 2.16×10^4 s to 4.32×10^4 s?

d[O2]/dT = -1/2 (0.500 – 0.250)/ (2.16×10^4 -4.32×10^4 )
= 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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