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
Step-by-step 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