The Reaction of NO Gas with H₂ Gas Has the Following

The reaction of NO gas with H₂ gas has the following rate law: Rate = k[H₂][NO]². A proposed mechanism is:
Step 1: H₂(g) + 2NO(g) $\rightarrow$ N₂O(g) + H₂O(g)
Step 2: N₂O(g) + H₂(g) $\rightarrow$ N₂(g) + H₂O(g)
What is the molecularity of steps 1 and 2, and which step is the slow, or rate-determining step?

A) 2; 2; step 1
B) 4; 4; step 2
C) 3; 2; step 1
D) 3; 2; step 2
E) Cannot be determined from the information provided.