Chemical reaction rate

The chemical reaction rate refers to the amount of the reactant concentration per unit time, or the increase in the concentration of the product, in a certain chemical reaction.

Single molecule reaction A B+D, then its reaction rate (first order reaction) is

v _k =- = = (1)

A negative sign before d[A]/dt indicates a decrease in the concentration of the reaction substance. Formula (1) is a differential form of the reaction rate. Since the concentration of the reactant varies with the progress of the reaction, a more general form of the above formula is the integral formula, which gives the concentration as a function of time. In this way, the degree of reaction at a given time can be determined, and the time required to reach a certain degree of reaction can be determined in turn. The integral equation can also be used to determine the rate constant k _{k of the} reaction. For example, for a first-order reaction, its differential is v _k =-dC/dt=k _k C, which can also become

Vk=- =-k _k dt (2)

Integral (2)

Then get k _k =- (3)

Or Ci=C ₀ (4)

Wherein the initial concentration of C ₀ -reactant;

C _i - the concentration of the reactant at time t;

k _k - the phase constant of the reaction kinetics, ie the rate constant of the reaction;

T-reaction time.

If C' _i represents the concentration of the product, that is, C ₀ -C' _i instead of C _i , then

k _k =- (5)

C' _i =C ₀ (1-e- ) (6)

For n-stage reactions, according to the law of mass action, it can be deduced and simplified to

v _k =- =k _k C ⁿ (7)

Formula (7) is applicable to reactions in which only one reactant is present, or there are several reactants having the same initial concentration. It is seen from the formula (7) that only the reaction rate of the zero-order reaction is independent of the concentration of the reactant. The table below lists the kinetic relationships with simple series reactions.

Dynamic equation with simple series reaction

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