Mass Action Flashcards
Mass action: Reaction rate depends on
– concentration of reactants
- higher concentrations give more collisions
– temperature
- higher temperature gives greater energy per collision
– Environment
- solvent
- pH
- catalysts
Based on experimental observations the law of mass
action states that:
the rate of a reaction (at a constant temperature) is proportional to the product of the concentrations of the reactants.
In order for a reaction to occur…
a collision must occur.
- The collision must be of sufficient energy to break the necessary bonds and be of proper orientation.
The number of collisions per unit time can be
expected to
change with the number of molecules of the reactants available.
At higher temperatures the number of
collisions is also expected to increase.
- That is, the rate varies as the concentrations
change
Reversible reactions: When two molecules A and B collide…
with one
another in an appropriate orientation, and with
sufficient energy, they can react to form new
molecules – the reaction products, say C and D:
A + B –> C + D
- The potential energy diagram for the bimolecular collision may have the following appearance:
Reversible reactions
As soon as significant concentrations of the product…
molecules C and D are formed, it will inevitably happen that a molecule of C will collide with a molecule of D. If these two molecules collide with one another in an appropriate orientation, and with sufficient energy, they can react to re-form the original
molecules A and B:
C + D –> A + B
- This event can be depicted on the potential energy diagram as:
Chemical reactions can take…
place not only in the forward direction but also in the reverse direction.
For an exothermic reaction the Ea …
(activation energy) for the reverse
reaction Ea,b is larger than the activation energy for the
forward reaction Ea,f.
Any reaction that can proceed to a significant extent
in both the forward and reverse directions is called a reversible
reaction.
*A reversible reaction is denoted as follows:
A + B <—> C + D