Problem: Consider the reaction of A(g) + B(g) + C(g) => D(g) for which the following data were obtained:Experiment Initial [A], mol/L Initial [B], mol/L Initial [C], mol/L Initial rate, mol/L.s1 0.0500 0.0500 0.0100 6.25 x 10-32 0.100 0.0500 0.0100 1.25 x 10-23 0.100 0.100 0.0100 5.00 x 10-24 0.0500 0.0500 0.0200 1.25 x 10-2What is the rate law of the reaction?

We’re being asked to calculate the rate law and the value of the rate constant (k) based on the reaction and data given.

A(g) + B(g) + C(g) → D(g)

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

$rate law = k {[A]}^{x} {[B]}^{y} {[C]}^{z}$

k = rate constant
A, B & C= reactants
x, y & z = reactant orders

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

Consider the reaction of A(g) + B(g) + C(g) => D(g) for which the following data were obtained:

Experiment Initial [A], mol/L Initial [B], mol/L Initial [C], mol/L Initial rate, mol/L.s

1 0.0500 0.0500 0.0100 6.25 x 10^-3

2 0.100 0.0500 0.0100 1.25 x 10^-2

3 0.100 0.100 0.0100 5.00 x 10^-2

4 0.0500 0.0500 0.0200 1.25 x 10^-2

What is the rate law of the reaction?