[Jackmcnulty]

Consider: A + 2B  C + 2D

It is asking me what the order of reaction with respect to B and A are. I understand the rate law that states

Rate = k[A]^mBⁿ

However I do not understand where the values for m and n are coming from.

We were also given tabulated data about [A]₀, and B₀ and Initial Δ[C]/Δt.

Is there something about this tabulated data that should tell me? Where B is not in brackets, the formatting messed it up and it is in fact the molarity of the reactant B.

[Orcio_87]

Rate = k[A]^mBⁿ

However I do not understand where the values for m and n are coming from.

Values "m" and "n" need to be calculated. If you have the data about concentration of A and B I suggest to draw a graph - concentration of A, B, C and D versus time of the reaction.

[Borek]

However I do not understand where the values for m and n are coming from.

Technically they reflect stoichiometry of the reaction as it happens - which sometimes, in the case of very simple reactions, is eactly what the reaction equation says, but in most cases they reflect so called elementary reactions - which are simpler steps towards the full, complete process, described by the balanced equation.

From the data you have you shoudl be probably able to determine m and n. It is often not trivial to do so, see Rate equation page in wikipedia.

[mjc123]

B in brackets is the format code for bold type. For concentration of B, you can just include a space, e.g. [B ].