We are asked to **determine by what factor does the reaction rate change if [B] is doubled (and the other reactant concentrations are held constant** given that a reaction in which A, B, and C react to form products is first order in A, second order in B, and zero-order in C.

We can calculate the reaction rate change of the reaction from its **rate law**.

Recall that the **rate law** only focuses on the reactant concentrations and has a general form of:

$\overline{){\mathbf{rate}}{\mathbf{}}{\mathbf{law}}{\mathbf{=}}{\mathbf{k}}{\left[\mathbf{A}\right]}^{{\mathbf{x}}}{\left[\mathbf{B}\right]}^{{\mathbf{y}}}}$

k = rate constant

A & B = reactants

x & y = reactant orders

From the given statement, we have:

x = 1

y = 2

hence we have the following rate law expression:

${\mathbf{rate}}{\mathbf{}}{\mathbf{law}}{\mathbf{=}}{\mathbf{k}}{\left[\mathbf{A}\right]}{{\left[\mathbf{B}\right]}}^{{\mathbf{2}}}$

A reaction in which A, B, and C react to form products is first order in A, second order in B, and zero order in C.

By what factor does the reaction rate change if [B] is doubled (and the other reactant concentrations are held constant)?