For the reaction 2N₂O₅(g) → 4NO₂(g) + O₂(g), the rate of formation of NO₂(g) is 2.8 × 10⁻⁷ Ms⁻¹. Calculate the rate of disappearance of N₂O₅(g).

For the reaction 2N₂O₅(g) → 4NO₂(g) + O₂(g), the rate of formation of NO₂(g) is 2.8 × 10⁻⁷ Ms⁻¹.

d[NO₂]/dt = 2.8 × 10⁻⁷ Ms⁻¹

The rate of disappearance of N₂O₅(g) is related to the rate of formation of NO₂(g) by the stoichiometry of the reaction.

From the balanced equation, 2 moles of N₂O₅ disappear for every 4 moles of NO₂ formed. Therefore:

-d[N₂O₅]/dt = (1/2) * d[NO₂]/dt

Substituting the given rate of formation of NO₂:

-d[N₂O₅]/dt = (1/2) * (2.8 × 10⁻⁷ Ms⁻¹)

-d[N₂O₅]/dt = 1.4 × 10⁻⁷ Ms⁻¹

The rate of disappearance of N₂O₅(g) is 1.4 × 10⁻⁷ Ms⁻¹.