For the reaction: 2N₂O₅(g) → 4NO₂(g) + O₂(g) the rate law is: = k[N₂O₅] At 300 K, the half-life is 2.50 × 10⁴ seconds and the activation energy is 103.3 kJ/mol O₂. At the time when N₂O₅ is being consumed at a rate of -1.2 × 10^-4 M/s, what is the rate at which NO₂ is being formed?

Question

Quizplus · Accepted Answer

The Answer of For the reaction: 2N₂O₅(g) → 4NO₂(g) + O₂(g) the rate law is: = k[N₂O₅] At 300 K, the half-life is 2.50 × 10⁴ seconds and the activation energy is 103.3 kJ/mol O₂. At the time when N₂O₅ is being consumed at a rate of -1.2 × 10^-4 M/s, what is the rate at which NO₂ is being formed?

For the Reaction: 2N2O5(g) → 4NO2(g) + O2(g) the Rate

For the Reaction: 2N₂O₅(g) → 4NO₂(g) + O₂(g) the Rate