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:
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?