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.
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.
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