For the reaction: 2 N₂O₅(g)→ 4 NO₂(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?

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The Answer of For the reaction: 2 N₂O₅(g)→ 4 NO₂(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: 2 N2O5(g)→ 4 NO2(g)+ O2(g)the Rate Law

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