Assuming 2O3 (g) → 3O2 (g), how much oxygen will be formed within 5.50 s for a reaction rate of 0.250 M/s?

Context: The rate of appearance of $\ce{O2}$ in the reaction: $\ce{2O3 (g) -> 3O2 (g)}$ is $\pu{0.250 M/s}$. So, over the first $\pu{5.50 s}$, will it form $\pu{1.38 M}$, or $\pu{4.13 M}$ of oxygen during the given time?


Which is right? Here are my solutions:


1. $\pu{0.250 M/s} \cdot \pu{5.50 s} = \pu{1.38 M}$
2. $\pu{0.250 M/s} \cdot \pu{5.50 s} \cdot 3 = \pu{4.13 M}$,
(3 in the calculation is the coefficient of the product in the reaction: $\ce{2 O3 (g) -> \mathbf{3} O2 (g)}$).


*I feel like the first one is right? I am overthinking this, and I need to make sure that I am doing this right.*


