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)?

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Rate Law concept. You can view video lessons to learn Rate Law. Or if you need more Rate Law practice, you can also practice Rate Law practice problems.