For the reaction: 2 N
2O
5(g) → 4 NO
2(g) + O
2(g) the rate law is:
=
k[N
2O
5]
At 300 K, the half-life is 2.50 × 10
4 seconds and the activation energy is 103.3 kJ/mol O
2. At the time when N
2O
5 is being consumed at a rate of 1.2 × 10
-4 M/s, what is the rate at which NO
2 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