At elevated temperatures, dinitrogen pentoxide decomposes to nitrogen dioxide and oxygen:. 2N2O5(g)→4NO2(g)+O2(g)
When the rate of formation of O2 is 8.1 x 10^−4 M/s, the rate of decomposition of N2O5 is M/s.
a. 3.2 x 10^−3
b. 8.1 x 10^−4
c. 1.6 x 10^−3
d. 2.0 x 10^−4
e. 4.1 x 10^−4

e. 4.1 x 10^−4

Explanation:

For the reaction;

2N2O5(g) → 4NO2(g) + O2(g)

The rate of formation is given as;

(1 / 4) Δ [O2] / Δt = (1 / 2 )Δ [N2O5] / Δt

Δ [O2] / Δt = 8.1 x 10^−4 M/s

Inserting into he equation, we have;

(1/4) (8.1 x 10^−4 ) = (1/2) (Δ [N2O5] / Δt)

2.025 x 10^−4 = (1/2) (Δ [N2O5] / Δt)

Δ [N2O5] / Δt = 2 * 2.025 x 10^−4

Δ [N2O5] / Δt  =  4.1 x 10^−4

Correct option is option E.

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