We’re being asked to determine the rate law for the reaction using the following data:

**A + B → C **

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

**We’re going to calculate the rate law and the rate constant using the following steps:**

What is the rate law for the reaction A + B → C? The following data were collected.

1. rate = 9.72 x 10^{-4} [A]^{0} [B]^{2}

2. rate = 5.6 x 10^{-3} [A]^{2} [B]^{0}

3. rate = 1.94 x 10^{-3} [A]^{0} [B]^{2}

4. rate = 4.67 x 10^{-3} [A]^{2} [B]^{1}

5. rate = 2.33 x 10^{-3} [A]^{0} [B]^{2}

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.