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Date: 19-7-2017
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Date: 17-12-2020
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Date: 19-12-2020
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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.
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