The decomposition of N2O5 is represented by the equation :2N2O5(g) →

1.	The decomposition of N2O5 is represented by the equation :2N2O5(g) → 4NO2(g) + O2(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» 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, = \(-\frac{1}{2}\)\(\frac{d[N_2O_5]}{dt}\) = \(\frac{1}{4}\)\(\frac{d[NO_2]}{dt}\) = \(\frac{d[O_2]}{dt}\)

The decomposition of N2O5 is represented by the equation :2N2O5(g) → 4NO2(g) + O2(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»

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,

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

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

= \(\frac{d[O_2]}{dt}\)

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