Indicate the order of reaction consistent with each observation. a. A plot of the concentration of the reactant versus time yields a straight line. Indicate the order of reaction consistent with each observation b. The reaction has a half-life that is independent of initial concentration. c. A plot of the inverse of the concentration versus time yields a straight line.

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For part (a), recognize that a plot of concentration versus time yielding a straight line indicates a zero-order reaction. In a zero-order reaction, the rate of reaction is constant and does not depend on the concentration of the reactant.

For part (b), understand that a reaction with a half-life independent of initial concentration is characteristic of a first-order reaction. In a first-order reaction, the half-life is constant and does not change with varying initial concentrations.

For part (c), identify that a plot of the inverse of concentration versus time yielding a straight line suggests a second-order reaction. In a second-order reaction, the rate is proportional to the square of the concentration of the reactant.

To summarize, the order of reaction can be determined by analyzing the relationship between concentration and time, as well as the behavior of the half-life.

These observations help in understanding the kinetics of the reaction and determining the rate law.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Zero-Order Reactions

In zero-order reactions, the rate of reaction is constant and does not depend on the concentration of the reactants. A plot of reactant concentration versus time yields a straight line with a negative slope, indicating that the concentration decreases linearly over time. This behavior is typical for reactions where a catalyst is saturated or when the reaction mechanism is limited by a surface reaction.

First-Order Reactions

First-order reactions are characterized by a rate that is directly proportional to the concentration of one reactant. The half-life of a first-order reaction is independent of the initial concentration, meaning it remains constant regardless of how much reactant is present. This relationship is crucial for understanding the kinetics of many biochemical and pharmaceutical processes.

Second-Order Reactions

Second-order reactions can involve either one reactant squared or two different reactants. A plot of the inverse of the concentration of the reactant versus time yields a straight line, indicating that the rate of reaction depends on the square of the concentration. This type of reaction often occurs in bimolecular processes, where two reactant molecules collide to form products.

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Second-Order Reactions

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Textbook Question

Consider the tabulated data showing the initial rate of a reaction (A → products) at several different concentrations of A. What is the order of the reaction? Write a rate law for the reaction including the value of the rate constant, k.

Textbook Question

The tabulated data were collected for this reaction: CH₃Cl(g) + 3 Cl₂(g) → CCl₄( g) + 3 HCl(g)

Write an expression for the reaction rate law and calculate the value of the rate constant, k. What is the overall order of the reaction?

Textbook Question

Indicate the order of reaction consistent with each observation.

a. The half-life of the reaction gets shorter as the initial concentration is increased.

b. A plot of the natural log of the concentration of the reactant versus time yields a straight line.

Textbook Question

Indicate the order of reaction consistent with each observation c. The half-life of the reaction gets longer as the initial concentration is increased.

Textbook Question

The tabulated data show the concentration of AB versus time for this reaction: AB( g)¡A( g) + B( g) Time (s) [AB] (M) 0 0.950 50 0.459 100 0.302 150 0.225 200 0.180 250 0.149 300 0.128 350 0.112 400 0.0994 450 0.0894 500 0.0812 Determine the order of the reaction and the value of the rate constant. Predict the concentration of AB at 25 s.

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