Final answer:
The rate of appearance of O₂ in the given reaction is 1.0 × 10⁻⁵ M/s.
Step-by-step explanation:
In the given reaction:
2NO₂(g) → 2NO(g) + O₂(g)
Since the stoichiometry of the reaction is 2:1 for NO₂ to O₂, the rate of appearance of O₂ is half the rate of disappearance of NO₂. Therefore, we need to calculate the rate of disappearance of NO₂ and divide it by 2 to find the rate of appearance of O₂.
The rate of disappearance of NO₂ can be calculated using the initial and final concentrations:
- Initial concentration: [NO₂]₀ = 0.0100 M
- Final concentration: [NO₂] = 0.00800 M
- Time: Δt = 100 s
Using the formula:
Rate of disappearance of NO₂ = ([NO₂] - [NO₂]₀) / Δt
Plugging in the values, we have:
Rate of disappearance of NO₂ = (0.00800 M - 0.0100 M) / 100 s = -0.00002 M/s
Finally, the rate of appearance of O₂ is half of the rate of disappearance of NO₂, so:
Rate of appearance of O₂ = -0.00002 M/s ÷ 2 = -0.00001 M/s = 1.0 × 10⁻⁵ M/s