Question

For the reaction, \[\ce{2N2O5_{(g)} -> 4NO2_{(g)} + O2_{(g)}}\]; ______ × Rate of disappearance of N₂O₅ = ______ × Rate of formation of NO₂.

Answer 1

For the reaction, \[\ce{2N2O5_{(g)} -> 4NO2_{(g)} + O2_{(g)}}\]; `bbunderline(1/2)` × Rate of disappearance of N₂O₅ = `bbunderline(1/4)` × Rate of formation of NO₂.

Explanation:

For a reaction:

\[\ce{aA -> bB}\]

The rate is written as

Rate = `- 1/a (d[A])/(dt) = 1/b (d[B])/dt`

Applying to the given reaction:

\[\ce{2N2O5 -> 4NO2 + O2}\]

So,

Rate = `-1/2 (d[N_2O5])/(dt)`

= `1/4 (d[NO_2])/(dt)`