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 2.2 × 10^-4 M/s, the rate of decomposition of N₂O₅ is ________ M/s.

Question

Quizplus · Accepted Answer

From the stoichiometry of the reaction, we can see that 2 moles of N2O5 decompose to produce 1 mole of O2. Therefore, the rate of decomposition of N2O5 is twice the rate of formation of O2. Thus, the rate of decomposition of N2O5 is 2.2 × 10-4 M/s * 2 = 4.4 × 10-4 M/s.

At Elevated Temperatures, Dinitrogen Pentoxide Decomposes to Nitrogen Dioxide and Oxygen