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?

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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=kAxBy[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:


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Problem Details

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?