Reaction quotient

In chemistry, a reaction quotient (Q_r) is a function of the activities or concentrations of the chemical species involved in a chemical reaction. In the special case that the reaction is at equilibrium the reaction quotient is constant and equal to the equilibrium constant which appears in the expression of the law of mass action.

A general chemical reaction in which α moles of a reactant A and β moles of a reactant B react to give σ moles of a product S and τ moles of a product T can be written as

αA + βB ⇌ σS + τT

The reaction is written as an equilibrium even though in many cases it may appear that all of the reactants on one side have been converted to the other side. When a mixture of A and B is made up and the reaction is allowed to occur, the reaction quotient, Q_r, is defined as:

$Q_r = \frac{\left\{S_t\right\}^\sigma \left\{T_t\right\}^\tau }{\left\{A_t\right\}^\alpha \left\{B_t\right\}^\beta }$

where {X_t} denotes the instantaneous activity of a species X at time, t. A compact general definition is (where П_j is the product across all j-indexed variables, and idem for П_i):

$Q_r=\frac{\prod_j a_{j}^{\nu_j}(t)}{\prod_i a_{i}^{\nu_i}(t)}$

where the numerator is a product of reaction product activities, a_j, each raised to the power of a stoichiometric coefficient, ν_j, and the denominator is a similar product of reactant activities. All activities refer to a time t.

As the reaction proceeds (assuming that there is no energy barrier to the reaction) with the passage of time the species' activities and hence the reaction quotient change. Eventually the activities become constant and the mixture is then said to be at equilibrium. The equilibrium constant, K, governs the final result via the relation

K = Q_r (t=∞),

although equilibrium will be effectively reached in a finite time in most reactions.

External links

Reaction quotient tutorials

• tutorial I
• tutorial II
• tutorial III