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)

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)

### Recently Asked Questions

- The following double integral cannot be solved as written. Reverse the order of integration to create a solvable equivalent intergal, and then solve it. Double

- Use a triple integral to find the volume of the region in between inverted cone whose equation is z = 2 − sqrt(x^2+y^2) , and the plane z = 0.

- If z(x, y) = e^( x^2 y) , with x = r cos θ and y = r sin θ, find the values of ∂z/∂r and ∂z/∂θ when r = 2 and θ = π/4.