The Experimental Rate Law for the Photochemical Decomposition of NO₂ $\to$

The experimental rate law for the photochemical decomposition of NO₂ to NO and O₂ is Rate = k[NO₂].Which of the following mechanisms is plausible? Justify your choice.
A)
Step 1: NO₂(g) $\to$ N(g)+ O₂(g)(slow)
Step 2: N(g)+ NO₂(g) $\to$ N₂O₂(g) (fast)
Step 3: N₂O₂(g) $\to$ 2 NO(g)(fast)
B)
Step 1: NO₂(g)+ NO₂(g) $\to$ NO₃(g)+ NO(g)(fast)
Step 2: NO₃(g) $\to$ NO(g)+ O₂(g)(fast)