Which of the following linear plots do you expect for a reaction A ⟶products if the kinetics are

step 1 So for the reaction of a species A forming products, if a is, if it's zero order in A, then if y

Which of the following linear plots do you expect for a...

Key Concepts

First-Order Kinetics

For a first-order reaction, the reaction rate is directly proportional to the concentration of the reactant. The integrated rate law is ln[Reactant] = ln[Reactant]_0 - kt, so when the natural logarithm of the reactant concentration is plotted against time, the resulting plot is linear with a slope of -k.

Zero-Order Kinetics

In a zero-order reaction, the reaction rate is constant and independent of the concentration of the reactant. The integrated rate law takes the form [Reactant] = [Reactant]_0 - kt, leading to a linear relationship when plotting reactant concentration versus time with a slope of -k.

Second-Order Kinetics

In a second-order reaction, where the reaction rate depends on the square of the reactant concentration (or the product of two reactant concentrations), the integrated rate law is generally given as 1/[Reactant] = 1/[Reactant]_0 + kt. Thus, plotting the reciprocal of the reactant concentration versus time yields a linear plot with a slope equal to k.

Reaction Orders

Reaction order indicates how the concentration of a reactant influences the rate of a reaction. Depending on whether a reaction is zero, first, or second order, the rate law changes, leading to different mathematical relationships that dictate how concentration decreases over time.

Integrated Rate Laws

Integrated rate laws are equations derived from differential rate laws that relate concentration and time for a given reaction order. They allow prediction of concentration at any time point and are used to determine the order of a reaction based on how the concentration data transforms into a linear plot.

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