# Problem: What is the rate law for the following mechanism in terms of the overall rate constant k? Step 1: A + B ↔ C (fast) Step 2: B + C → D (slow)

###### FREE Expert Solution

We’re asked to determine the overall rate constant K for the given two steps mechanism.

When a reaction mechanism is given, the rate law will depend on reactants and products in the slow step.

Rate law only involves the reactants
The coefficients of the reactants in the slow step are the order of the reaction with respect to that reactant
Rate Law has a general form of:

Where

k = rate constant

X & Y = reactants

a & b = reactant orders

The equilibrium constant has a general form of:

$\overline{){{\mathbf{K}}}_{{\mathbf{r}}}{\mathbf{=}}\frac{\mathbf{p}\mathbf{r}\mathbf{o}\mathbf{d}\mathbf{u}\mathbf{c}\mathbf{t}\mathbf{s}}{\mathbf{r}\mathbf{e}\mathbf{a}\mathbf{c}\mathbf{t}\mathbf{a}\mathbf{n}\mathbf{t}\mathbf{s}}}$

###### Problem Details

What is the rate law for the following mechanism in terms of the overall rate constant k?

Step 1: A + B ↔ C (fast)

Step 2: B + C → D (slow)