Question

Consider the decomposition of N₂O_5(g) to form NO_2(g) and O_2(g) . At a particular instant N₂O₅ disappears at a rate of 2.5 x 10^-2 mol dm^-3 s^-1 . At what rates are NO₂ and O₂ formed? What is the rate of the reaction?

Answer 1

2N₂O_5(g) → 4NO_2(g) + O_2(g)

from the stoichiometry of the reaction.

Rate of disappearance of N₂O₅ is 2.5 x 10^-2 mol dm^-3s^-1

∴ The rate of formation of NO₂ at this temperature is 2 x 2.5 x 10^-2 = 5 x 10^-2 mol dm^-3 s^-1