Integrated Rate Equations for Zero and First Order An integrated rate equation provides a mathematical expression that relates the concentration of reactant...
Integrated Rate Equations for Zero and First Order
An integrated rate equation provides a mathematical expression that relates the concentration of reactants or products at different times in a chemical reaction. These equations are particularly useful when determining the rate of a reaction, as they allow us to directly integrate the concentration of reactants or products over time.
Zero Order
In a zero-order reaction, the rate of the reaction is independent of the concentration of the reactants. This means that the concentration of reactants does not affect the rate of the reaction. For example, the reaction between hydrogen and oxygen to form water is a zero-order reaction.
First Order
In a first-order reaction, the rate of the reaction is proportional to the concentration of the reactant. This means that the rate of the reaction increases as the concentration of the reactant increases. For example, the reaction between hydrochloric acid and sodium hydroxide to form sodium chloride and water is a first-order reaction.
The integrated rate equations for zero and first-order reactions are:
Integrated Rate Equation for Zero Order:
where [A] is the concentration of the reactant, k is the rate constant.
Integrated Rate Equation for First Order:
where [A] is the concentration of the reactant, k is the rate constant, and k_2 is a second-order rate constant.
These integrated rate equations allow us to calculate the rate of a reaction by integrating the concentration of reactants or products over time. This information can be used to predict the rate of a reaction under different conditions