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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
Textbook 
General Chemistry: Principles and Modern Applications

General Chemistry: Principles and Modern Applications


Edition: 11th
Authors:
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