Two reaction schemes are kinetically equivalent if they imply the same
rate law. For example, consider the two schemes (i) and (ii) for the formation of C from A:
Providing that B does not accumulate as a
reaction intermediate.
Providing that B does not accumulate as a
reaction intermediate:
Both equations for
![d [ C ] d t](../../mathml/K03403-4.png)
are of the form:
where
and
are constants (sometimes called '
coefficients in the rate equation'). The equations are identical in their dependence on concentrations and do not distinguish
whether
OH−
catalyses the formation of B, and necessarily also its reversion to A, or is involved
in its further
transformation to C. The two schemes are therefore kinetically equivalent under conditions to which
the stated provisos apply.
Source:
PAC, 1994, 66, 1077
(Glossary of terms used in physical organic chemistry (IUPAC Recommendations 1994))
on page 1133
Cite as:
IUPAC. Compendium of Chemical Terminology, 2nd ed. (the "Gold Book"). Compiled by
A. D. McNaught and A. Wilkinson. Blackwell Scientific Publications, Oxford (1997).
XML on-line corrected version: http://goldbook.iupac.org (2006-) created by M. Nic,
J. Jirat, B. Kosata; updates compiled by A. Jenkins. ISBN 0-9678550-9-8.
https://doi.org/10.1351/goldbook.
![d [ C ] d t = k 1 k 2 [ A ] [ OH − ] k 2 + k −1 [ OH − ]](../../mathml/K03403-1.png){kind=small}
![d [ C ] d t = k 1 k 2 [ A ] [ OH − ] k −1 + k 2 [ OH − ]](../../mathml/K03403-3.png){kind=small}
![d [ C ] d t = r [ A ] [ OH − ] 1 + s [ OH − ]](../../mathml/K03403-5.png){kind=small}
