# Order Of Reaction [closed]

A+B ———> C+D

If A and B are taken in excess then what will be the order of reaction?

I thought since it is taken in excess, their change wont really be significant and so answer would be 0.

• Having both A and B in excess makes no sense. There are only three possible cases. (1) A > B, (2) A = B, or (3) A<B. If (1) Then A is in excess. If (3) then B is in excess.
– MaxW
Nov 11, 2018 at 18:55
• Reaction orders are not related to excesses at all. The question is wrong in its premises. Nov 11, 2018 at 19:23
• No like pseudo kind of rate order@IvanNeretin Nov 11, 2018 at 19:25
• If the reaction is a kind of heterogeneous catalytic reaction or photochemical reaction your answer correct Nov 15, 2018 at 7:22

3 doesn't make any sense for the reaction order.

Given the elementary reaction

$$\ce{aA + bB -> \text{products}}$$

then the rate equation would be

$$r = k\ce{[A]^a[B]^b}$$

since by definition an elementary reaction is a reaction for which the stoichometric coefficients are the same as exponents for the concentrations in the rate equation. Thus the order of the reaction is $$a+b$$.

So for the case of the elementary reaction

$$\ce{A + B -> \text{products}}$$

$$a=1$$ and $$b=1$$ so the reaction order is 2.

Reaction orders are defined per component. If both A and B are in excess (but available in roughly the same concentration), the reaction order would be one in either of them.

If A or B is in excess, then the reaction order is one for the compound in excess and zero for the other compound.