Zero-Order Reactions

Zero-order reaction rates occur when the rate of reactant disappearance is independent of reactant concentrations. The differential rate law for the hypothetical zero-order reaction E → F could be written as:

Rate of reaction = – [latex] frac{Delta [E]}{Delta t} [/latex] =[latex] extit{ k} [/latex]

The integrated rate law can be written in the form of a straight line as:

[latex] [E]{}_{t}{}_{ } [/latex]= –[latex] extit{k}t + [E]{}_{0} [/latex]

 Therefore, if the reaction is zero order, a plot of [E] versus t will produce a straight line with a slope that corresponds to the negative of the product of the rate constant and time, –kt, and a y-intercept that corresponds to the initial concentration, [E]₀ (Figure 1.1. “Concentration vs. Time, Zero-Order Reaction”).

Figure 1.1. Concentration vs. Time, Zero-Order Reaction

The graph shows the plot of concentration versus time for a zero-order reaction.