Instantaneous Rate of Decomposition

Question

Given the decomposition of

𝐻_2𝑂_2: 𝐻_2𝑂_2→ 2 𝐻_2𝑂 + 𝑂_2

the instantaneous rate of decomposition of hydrogen peroxide at t = 10.8 hr is determined to be 1.20 𝑥 10−2 M/hr, that is:

-∆ {H_2O_2}/ ∆t=1.20*10^-2

Calculate the instantaneous rate of production of water in M/hr.

Answer 1

H₂O₂ + H₂O₂ ==> 2H₂O + O₂

2H₂O₂ ==> 2H₂O + O₂ .. balanced equation for decomposition of hydrogen peroxide

For each mole of H₂O₂ that decomposed, we obtain one mole of H₂O as product

Thus if instantaneous rate of decomposition of H₂O₂ = 1.20x10^-2 M/hr, the rate of production of H₂O = 1.20x10^-2 M/hr.