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?

FREE Expert Solution

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:

$\boxed{\mathbf{rate}\mathbf{ }\mathbf{law}\mathbf{=}\mathbf{k}{\left[\mathbf{A}\right]}^{\mathbf{x}}{\left[\mathbf{B}\right]}^{\mathbf{y}}{\mathbf{\left[}\mathbf{C}\mathbf{\right]}}^{\mathbf{z}}}$

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:

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