Question

The decomposition of N₂O₅ is represented by the equation :

2N₂O_5(g) → 4NO_2(g) + O_2(g)

(a) How is the rate of formation of NO₂ related to the rate of formation of O₂?

(b) How is the rate of formation of O₂ related to the rate of consumption of N₂O₅?

Answer 1

Given :

2N₂O_5(g) → 4NO_2(g) + O_2(g)

(a) Rate of formation of NO₂ at time,

t = \(\frac{d[NO_2]}{dt}\)

Rate of formation of O₂ at time,

t = \(\frac{d[O_2]}{dt}\)

They are related to each other through rate of reaction.

∴ Rate of reaction = \(\frac{1}{4}\)\(\frac{d[NO_2]}{dt}\)\(\frac{d[O_2]}{dt}\)

(b) Rate of consumption of N₂O₅ at time t,

= \(-\frac{d[N_2O_5]}{dt}\)

Rate of reaction,

= \(-\frac{1}{2}\)\(\frac{d[N_2O_5]}{dt}\) 

= \(\frac{d[O_2]}{dt}\)

In general,

Rate of reaction,

= \(-\frac{1}{2}\)\(\frac{d[N_2O_5]}{dt}\)

= \(\frac{1}{4}\)\(\frac{d[NO_2]}{dt}\) 

= \(\frac{d[O_2]}{dt}\)