For rate equations, are AB+A vs 2A+B vs A2+B equivalent?
I.e. if the reaction is dependent on the concentrations of A, do all three of the above give rate=k[A]2.
I think they would NOT be equal as A is a concentration.
For example, if A=0.5 moles/L
- A2=A*A (I think?)=0.5*0.5=0.25
- Note sure how to treat AB
FYI, for some context, here is the problem I am working on
I can see the slow reaction in the bottom left box has A+2B - so it is NOT of the form rate=k[A]2[ B]
In the bottom right one we have 2A+B -> D+I , so the rate equation iS of the form rate=k[A]2B
However, in the top right one, We have A2+B -> A2B.
I do not know if this A2, where it is 1 molecule containing 2 A atoms is equivalent to the bottom right one where we had 2 moles of A)
Similarly for the top left one, I do not know what to do when it is AB rather than A and B separately.
Thanks for the help.