The notes in my study guide say:
In the rate law the order of reaction with respect to a reactant indicates how many molecules of that reactant participate in the rate-determining step.
If a reactant is first order, one molecule reacts in the rds.
If a reactant is second order, two molecules react in the rds.
example:
H2 (g) + 2ICl (g) --> I2 (g) + 2HCl (g)
rate = [H2][iCl]
The stoichiometric equation tells us that overall, 1 molecule of H2, reacts with 2 molescules of ICl to give the products. But it does not tell us about the individual steps which make up the overall reaction. There is no link between the stoichiometric equation and the reaction mechanism or the rate equation.
The rate equation tells us that the rate-determining step involves 1 molecule of H2 and and 1 molecule of ICl, because it is a first order with respect to both.