Reaction Rates

Consider a general reaction,

              (1.1)

We describe the rate of the reaction in terms of the rate of disappearance of one of the reactants or the rate of appearance of the product,

The stoichiometry of the reaction tells us that in time interval Δt, Δ[B] = 3 Δ[A], Δ[C] = - 2 Δ[A]; furthermore, Δ[A] and Δ[B] are negative, Δ[C] is positive. Thus we must include an appropriate sign and stoichiometric coefficient in expressing the rate of the reaction:

           (1.2)

It is most common to express rates in terms of molar concentrations of species, even for gas-phase reactions. The usual units of a reaction rate are mol L^-1s^-1.

When a reaction is slow enough, it is appropriate to express the rate as the ratio of a concentration change, Δ[A], to a time interval, Δt, but when the reaction is faster, we consider the limit as Δt approaches zero, the first derivative of [A] with respect to time:

                            (1.3)

مواضيع ذات صلة

The Molecular Interpretation of Entropy

Spontaneous Change

Biological Catalysts

Homogeneous Catalysts

Heterogeneous Catalysts

The Rate-Determining Step

Multistep Mechanisms

Elementary Steps and Rate Laws

Elementary Steps

Half-Life

Graphical Methods for Determining Reaction Order

Zero-Order Reactions