At 40 degrees Celsius CH2O2(aq) will decompose according to the following reaction: 2H2O2(aq) =– 2H2O(l) + O

Question

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 x 10^4 s. Use this rate to calculate the average rate of production of O2(g) over the same time period.
b. What are these rates for the time period 2.16 3 x10^4 s to 4.32 x 10^4 s?

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Kim Chi 2 months 2021-07-15T16:59:58+00:00 1 Answers 4 views 0

Answers ( )

    0
    2021-07-15T17:01:53+00:00

    Answer:

    A. Rate of decomposition of H₂O₂ = 2.31 × 10-⁵ M/s

    Average rate of production of O₂ = 1.16 × 10-⁵ M/s

    B. Rate of decomposition of H₂O₂ = 1.16 × 10-⁵ M/s

    Average rate of production of O₂ = 5.8 × 10-⁶ M/s

    Explanation:

    The rate of a reaction is defined as the number of moles of reactant converted or the product formed per unit time.

    Reaction rate = change in the concentration of product or reactant / time taken for the change.

    A. i) For the decomposition of H₂O₂, the reaction equation is given below:

    2 H₂O₂ (aq) —-> 2 H₂O (l) + O₂ (g)

    a. the average rate of decomposition of H2O2 between 0 and 2.16 x 10^4 s is calculated as follows :

    Rate of decomposition of H₂O₂ = change in concentration / change in time

    Rate of decomposition of H₂O₂ = (0.500 – 1.000) M / (2.16 × 10⁴ – 0) s = 2.31 × 10-⁵ M/s

    ii) The mole ratio of O₂ to H₂O₂ = 1 : 2 = 0.5

    Average rate of production of O₂ = 0.5 × rate of decomposition of H₂O₂

    Average rate of production of O₂ = 0.5 × 2.31 × 10-⁵ M/s = 1.16 × 10-⁵ M/s

    B. The rate of decomposition of H₂O₂ for the time period 2.16 3 x10^4 s to 4.32 x 10^4 s is calculated as follows:

    Rate of decomposition of H₂O₂ = change in concentration / change in time

    Rate of decomposition of H₂O₂ = (0.250 – 0.500) M / ( 4.32 × 10⁴ – 2.16 × 10⁴) s = 1.16 × 10-⁵ M/s

    ii) The mole ratio of O₂ to H₂O₂ = 1 : 2 = 0.5

    Average rate of production of O₂ = 0.5 × rate of decomposition of H₂O₂

    Average rate of production of O₂ = 0.5 × 1.16 × 10-⁵ M/s = 5.8 × 10-⁶ M/s

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