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

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

anonymous · Answer

2.4 x 10-4 M/s

chenping · Answer

I thought this is a chemistry qs? haha..