For the reaction: 2 N2O5(g) 4 NO2(g) + O2(g) the rate law is: = ...

[aabwk4]

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?
◦ 1.2 × 10^-4 M/s
◦ 2.4 × 10^-4 M/s
◦ 6.0 × 10^-5 M/s
◦ 3.0 × 10^-5 M/s
◦ 4.8 × 10^-4 M/s

[perkiness]

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[aabwk4]

Thanks for the timely response, appreciate it

[AmberC1996]

YES! Correct, THANKS for helping me on my review