Question

For the reaction: N2O5(g) \longrightarrow⟶ 2NO2(g) + 1/2O2(g)

If N2O5 is decomposing with an instantaneous rate of 7.81 mol/L·s, what is the instantaneous rate of formation of NO2?
I don't know where to begin

Answer 1

The given equation from the problem above is already balance,
N2O5 ---> 2NO2 + 0.5O2
Since, in every mole of N2O5 consumed, 2 moles of NO2 are formed, we can answer the problem by multiplying the given rate, 7.81 mol/L.s with the ratio.
(7.81 mol/L.s) x (2 moles NO2 formed/ 1 mole of N2O5 consumed)
= 15.62 mol/L.s
The answer is the rate of formation of NO2 is approximately 15.62 mol/L.s.