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Chapter 16: Problem 9

Explain how a graph can be useful in defining and measuring the rate of a chemical reaction.

Short Answer

Expert verified
Graphs are useful in defining and measuring the rate of a chemical reaction as they visually depict the change in concentration of reactants or products over time. This visualization makes it clear, at a glance, how quickly a reaction takes place, how the rates alter over time, and the impact of factors like temperature and concentration. The slope or gradient of the curve in the graph provides the reaction rate. Therefore, graphs serve as essential tools in chemical kinetics, aiding in better comprehension and analysis of reaction rates and mechanisms.

Step by step solution

01

Understanding the concept of reaction rate

The rate of a chemical reaction refers to the speed at which the reactants are converted into products. It's usually measured in terms of change in concentration of reactants or products over time (for example, mol/L/s).
02

Representing reaction rate on graphs

A graph offers a visual way to track these changes over time. The most common type of graph used in this scenario is a concentration-time graph, where the x-axis represents time (usually in seconds, minutes or hours), and the y-axis represents the concentration of the reactants or products (usually in mol/L or similar units).
03

Utility of Graphs in measuring reaction rates

From these graphs, the rate of the chemical reaction is usually determined by the gradient or the slope of the curve. A steeper slope indicates a faster reaction. The rate could also be determined at any particular moment (instantaneous rate) or over the entire reaction (average rate).
04

Exploring the benefits of using graphs

These graphs allow scientists and students to easily visualize the progress of a reaction over time, compare rates between different reactions, and understand patterns and trends related to factors like temperature, concentration, and catalysts. They also help determine the order of the reaction and evaluating rate laws and rate constants of a reaction.

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Most popular questions from this chapter

Why is it necessary, in defining the rate of a reaction, to require that \(\Delta t\) be small?

Explain the effect that area has on reactions that occur on surfaces.

Define reaction rate.

In the reaction $$2 \mathrm{NO}(g)+\mathrm{Br}_{2}(g) \rightarrow 2 \mathrm{NOBr}(g)$$ doubling the \(\mathrm{Br}_{2}\) concentration doubles the rate, but doubling the NO concentration quadruples the rate. Write the rate law.

Why is it necessary to divide by the coefficient in the balanced chemical equation when calculating a reaction rate? When can that step be omitted?
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