The rate law for the reaction shown below is given by rate = k[NO][Cl2].
2 NO(g) + Cl2(g) → 2 NOCl(g)
(a) What is the order of the reaction?
firstsecond thirdfourth
(b) A mechanism involving the following steps has been proposed for the reaction.
NO(g) + Cl2(g) → NOCl2(g)
NOCl2(g) + NO(g) → 2 NOCl(g)
If this mechanism is correct, what does it imply about the relative rates of these two steps?
The second reaction must be the rate determining (slow) step and the first reaction is faster.The first reaction must be the rate determining (slow) step and the second reaction is faster.
