No. Think about it like this:
For each mole of reaction, 1 mole of I2 is consumed, and 2 moles of N3- are consumed. So the rate of consumption of N3- is twice that of I2:
d[N3-]/dt = 2 d[I2]/dt
So if we define the rate of reaction as the rate of consumption of I2, then
rate = -d[I2]/dt = -1/2 d[N3-]/dt - i.e. you divide by the stoichiometric coefficient, not multiply.
So if the rate of the RDS is r' = -d[N3-]/dt
then rate of reaction r = 1/2 r'.
I strongly dislike this "reaction rate r" language, though I suppose if your textbook or prof uses it, you have to go with it. I much prefer to talk about the rate of change of a specific reagent (e.g. -d[I2]/dt), and keep this in view throughout the calculation. That's how we did kinetics when I learnt it, many moons ago. I think it is easier this way to avoid confusion.