Rate equation

Relation between chemical reaction rate and concentrations of the reactants

In chemistry, the rate equation (also known as the rate law or empirical differential rate equation) is an empirical differential mathematical expression for the reaction rate of a given reaction in terms of concentrations of chemical species and constant parameters (normally rate coefficients and partial orders of reaction) only. For many reactions, the initial rate is given by a power law such as v 0 = k [ A ] x [ B ] y {\displaystyle v_{0}\;=\;k[\mathrm {A} ]^{x}[\mathrm {B} ]^{y}} where ⁠ [ A ] {\displaystyle [\mathrm {A} ]} ⁠ and ⁠ [ B ] {\displaystyle [\mathrm {B} ]} ⁠ are the molar concentrations of the species ⁠ A {\displaystyle \mathrm {A} } ⁠ and ⁠ B , {\displaystyle \mathrm {B} ,} ⁠ usually in moles per liter (molarity, ⁠ M {\displaystyle M} ⁠). The exponents ⁠ x {\displaystyle x} ⁠ and ⁠ y {\displaystyle y} ⁠ are the partial orders of reaction for ⁠ A {\displaystyle \mathrm {A} } ⁠ and ⁠ B {\displaystyle \mathrm {B} } ⁠, respectively, and the overall reaction order is the sum of the exponents.

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