Calculating average rate of decomposition

Question

Assignment:

Question 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?

Question 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)

Question 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

Question 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)

Provide complete and step by step solution for the question and show calculations and use formulas.