Question
the formation of no(g) from n2 and o2 has the following proposed mechanism.
N2 (g) + O2 (g) -> 2 NO (g)
step 1 O2 <=> 2O (fast eq)
step 2 O + N2 -> NO + N (slow)
step 3 N + O -> NO (fast)
The experimentally determined rate law for this would be:
1. Rate = kobs (N2)(o2)^1/2
2. Rate = kobs (N2)(O2)
3. Rate = kobs (N2)
4. Rate = kobs (O2)^2
N2 (g) + O2 (g) -> 2 NO (g)
step 1 O2 <=> 2O (fast eq)
step 2 O + N2 -> NO + N (slow)
step 3 N + O -> NO (fast)
The experimentally determined rate law for this would be:
1. Rate = kobs (N2)(o2)^1/2
2. Rate = kobs (N2)(O2)
3. Rate = kobs (N2)
4. Rate = kobs (O2)^2