At elevated temperatures, dinitrogen pentoxide decomposes to nitrogen dioxide and oxygen: 2n2o5(g) → 4no2 (g) + o2 (g) when the rate of formation of no2 is 5.5 ⋅ 10-4 m/s, the rate of decomposition of n2o5 is m/s. at elevated temperatures, dinitrogen pentoxide decomposes to nitrogen dioxide and oxygen: 2n2o5(g) 4no2 (g) + o2 (g) when the rate of formation of no2 is 5.5 10-4 m/s, the rate of decomposition of n2o5 is m/s. 2.8 ⋅ 10-4 1.4 ⋅ 10-4 5.5 ⋅ 10-4 10.1 ⋅ 10-4 2.2 ⋅ 10-3

The rate of descomposition of N₂O₅ is: 2,8 M/s

Explanation:

The global reaction is:

2 N₂O₅ (g) → 4 NO₂ (g) + O₂ (g)

The problem says that rate of formation of NO₂ = 5,5x10⁻⁴ M/s where M is molarity --

The rate of descomposition of N₂O₅ is:

5,5x10⁻⁴ × = 2,8 M/s

I hope it helps!

Answer :  The rate of decomposition of is

Explanation : Given,

Rate of formation of =

The given rate of reaction is,

The expression for rate of reaction :

Now we have to calculate the rate of decomposition of .

As we know that,

So,

Thus, the rate of decomposition of is