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Mass action
Mass action in science is the idea that a large number of small units (especially atoms or molecules) acting randomly by themselves can in fact have a larger pattern. For example, consider a cloud of gas is moving in a given direction. Individual molecules will move in a semi-random walk, but if taken as a whole, they have direction.
The Law of Mass Action, first expressed by Waage and Guldberg in 1864 (Waage, P.; Guldberg, C. M. Forhandlinger: Videnskabs-Selskabet i Christiana 1864, 35) states that the speed of a chemical reaction is proportional to the quantity of the reacting substances. More formally the change of a product quantity is proportional to the product of reactant activities. In the case of a reaction occurring in a gas phase, the activities are equal to the partial pressures. In the case of a well-stirred aqueous medium, the activities are equal to the concentrations. Therefore, if we have a reaction:
The speed of A2B formation is ![\frac{d[A_2B]}{dt} = k \times [A]^2 \times [B]](a/../upload/math/71d5dc2559546561babafb36769f9738.png)
where k is a constant.
A general case is given by a reversible reaction such as:
with
![\frac{d[C]}{dt} = k_{AB} \times [A]^2 \times [B] - k_{CD} \times [C] \times [D]](a/../upload/math/14db24aea368f8a88176ef2a02ca3db6.png)
Which means C and D are produced by the onward reaction, and consumed by the backward reaction. A consequence of the Mass Action Law is that after a sufficient amount of time, there will be an equilibrium between the two reactions and:
![k_{AB} \times [A]2 \times [B] = k_{CD} \times [C] \times [D]](a/../upload/math/d5c5b2b37e2c85159e62721226b670e1.png)
resulting in the following equation, often called Mass Action Law itself
![K = \frac{[C][D]}{[A]^2[B]} = \frac{k_{AB}}{k_{CD}}](a/../upload/math/ffe2469769225a1ed79f0634236a85f8.png)
See also
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