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Ch.14 - Chemical Kinetics
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
All textbooksBrown 14th EditionCh.14 - Chemical KineticsProblem 4b
Chapter 14, Problem 4b

Suppose that for the reaction K + L → M, you monitor the production of M over time, and then plot the following graph from your data:
Graph showing the concentration of M over time, indicating reaction progress for K + L → M.
(b) Is the reaction completed at t = 15 min? [Section 14.2]

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Observe the graph showing the concentration of M over time.
Note that the concentration of M increases linearly from 0 to 30 minutes.
At 30 minutes, the concentration of M levels off and remains constant.
Determine if the reaction is complete by checking if the concentration of M changes after 15 minutes.
Since the concentration of M continues to increase after 15 minutes and only levels off at 30 minutes, the reaction is not complete at t = 15 min.

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Key Concepts

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

Reaction Completion

A chemical reaction is considered complete when the concentration of the products no longer changes over time. In the context of the provided graph, this means that if the concentration of M remains constant after a certain time, the reaction has reached completion.
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Rate of Reaction

The rate of a chemical reaction refers to how quickly reactants are converted into products. This can be observed in the graph as the slope of the line representing the concentration of M over time. A steeper slope indicates a faster reaction rate, while a flat line indicates that the reaction has slowed or stopped.
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Equilibrium

Chemical equilibrium occurs when the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products. In the graph, if the concentration of M stabilizes at a certain level, it suggests that the system may have reached equilibrium, indicating that the reaction is no longer proceeding in either direction.
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Related Practice
Textbook Question

The following diagrams represent mixtures of NO(g) and O21g2. These two substances react as follows: 2 NO1g2 + O21g2¡2 NO21g2 It has been determined experimentally that the rate is second order in NO and first order in O2. Based on this fact, which of the following mixtures will have the fastest initial rate? [Section 14.3]

Textbook Question

You study the rate of a reaction, measuring both the concentration of the reactant and the concentration of the product as a function of time, and obtain the following results:

Which chemical equation is consistent with these data: (i) A → B, (ii) B → A, (iii) A → 2 B, (iv) B → 2 A?

Textbook Question

Consider the following graph of the concentration of a substance X over time. Is each of the following statements true or false? (d) As time progresses, the curve will eventually turn downward toward the x-axis. [Section 14.2]

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Textbook Question

Given the following diagrams at t = 0 min and t = 30 min

After four half-life periods for a first-order reaction, what fraction of reactant remains? [Section 14.4]