For a reaction: $\ce{aA->product}$
The rate law is $\text{Rate}=-\dfrac{\mathrm d[A]}{a\,\mathrm dt} = k$
Where:
- $k$ is the rate constant
- $[\ce{A}]$ is the concentration of the reactant $\ce{A}$ in the reaction
- $a$ is the stoichiometric coefficient of $\ce{A}$
If we integrate the relation, we get:
$$[\ce{A}]-[\ce{A}]_0=-akt $$
However, my instructor wrote the relation on board as below;
$$[\ce{A}]-[\ce{A}]_0=-kt$$
Why is $a$ not needed in the integrated rate law?