Can anyone please help me answer this chemistry question?

Question

a) What is the rate law of a reaction that is zeroth-order with respect to [A], first order with respect to [B], and second-order with respect to [C].

b) Determine the effect on the overall reaction rate (be as specific as possible) if you were to half the concentration of A, and double the concentrations of B and C? Justify the answer with reference to each reactant’s effect on the overall reaction rate, as well as the overall rate change.

Answer 1

Well, since you didn't really provide a particular reaction, we will assume you have the following:

A + B + C ==> Products

rate = k[A]⁰[B]¹[C]² or...

rate = k[B][C]²

b)

halving the [A] will have no effect on the overall rate of reaction since it is zero order with respect to A, and [A] therefore doesn't appear in the rate law. Doubling [B] will double the rate since it is first order with respect to B, and doubling [C] will increase the rate 4 times because it is 2nd order with respect to C. The overall rate change will be 2 x 4 = 8 times faster.