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Chapter 2: Problem 31

How are the reactions classified on the basis of rates of reactions? Give examples.

Short Answer

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Question: What are the three classifications of reactions based on their rates, and provide an example for each classification. Answer: The three classifications of reactions based on their rates are: 1. Fast reactions: These occur rapidly, often within fractions of a second, and usually release large amounts of energy. For example, the combustion of hydrogen in air: \[2H_2(g) + O_2(g) \rightarrow 2H_2O(g)\] 2. Moderate reactions: These reactions take place at a noticeable but not extremely rapid pace, lasting from a few seconds to several minutes. For example, the precipitation of silver chloride from its soluble components: \[AgNO_3(aq) + NaCl(aq) \rightarrow AgCl(s) + NaNO_3(aq)\] 3. Slow reactions: These reactions take a considerable amount of time to occur, from a few hours to days, months, or even years. For example, the formation of rust on iron in the presence of water and oxygen: \[4Fe(s) + 3O_2(g) + 6H_2O(l) \rightarrow 4Fe(OH)_3(s)\]

Step by step solution

01

Understanding Reaction Rates

Reaction rates refer to the speed at which reactants are transformed into products in a chemical reaction. The rate of a reaction is influenced by various factors, such as temperature, pressure, concentration of reactants, and presence of catalysts. Reactions can be classified into three categories based on their rates: fast reactions, moderate reactions, and slow reactions.
02

Fast Reactions

Fast reactions are chemical reactions that occur rapidly, often within fractions of a second. Many fast reactions release large amounts of energy, such as heat, light, or sound. The high energy release is usually a consequence of highly reactive substances being involved in the reaction. Example: Combustion of hydrogen in air: \[2H_2(g) + O_2(g) \rightarrow 2H_2O(g)\] This reaction is a fast reaction that generates heat and water vapor. Fast reactions are often used in applications where rapid energy release is desirable, such as in explosives or rocket propulsion.
03

Moderate Reactions

Moderate reactions are chemical reactions that take place at a noticeable but not extremely rapid pace. These reactions might last from a few seconds to several minutes. Examples of moderate reactions can be found in everyday life processes, such as the breakdown of glucose to produce energy in the human body or the ripening of fruit. Example: Precipitation of silver chloride from its soluble components: \[AgNO_3(aq) + NaCl(aq) \rightarrow AgCl(s) + NaNO_3(aq)\]
04

Slow Reactions

Slow reactions are chemical reactions that take a considerable amount of time to occur, lasting from a few hours to days, months, or even years. Slow reactions are usually accompanied by a gradual change in the properties of the reacting substances. Examples of slow reactions include corrosion and biological growth. Example: Formation of rust on iron in the presence of water and oxygen: \[4Fe(s) + 3O_2(g) + 6H_2O(l) \rightarrow 4Fe(OH)_3(s)\] In summary, reactions can be classified into fast, moderate, and slow reactions based on their rates of reactions. Fast reactions happen quickly and often release large amounts of energy, moderate reactions are noticeable but not overly rapid, and slow reactions take a long time to occur with gradual changes in the reacting substances' properties.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Fast Reactions
Fast reactions are those that take place in a very short time, often mere seconds or even less. These reactions can generally be observed because they release energy quickly and visibly, in the form of heat, light, or sound. An example of a fast reaction is the combustion of hydrogen gas, where hydrogen reacts with oxygen to form water vapor. The speed and vigor of fast reactions make them pivotal in various applications, such as in the propulsion systems of rockets and in explosives. Because of the immediate energy release, these reactions are used where fast transformation of energy is necessary.
Moderate Reactions
Moderate reactions occur at a pace that can usually be perceived without instrumentation over a short time span, often from a few seconds to several minutes. They are not as explosive or immediate as fast reactions but are manifestly quicker than slow ones. An everyday example includes the breakdown of glucose in our bodies to provide energy or the ripening of fruits. These reactions are noticeable but not instantaneous, offering a more controlled and sustained release of energy or change of state. Such reactions are beneficial for processes needing a steady and manageable pace.
Slow Reactions
Slow reactions extend over much longer periods, from several hours to even years. These reactions are typically characterized by gradual changes and transformations. One classic example is the rusting of iron, which occurs when iron slowly combines with oxygen and water over time, forming iron hydroxide. Slow reactions are crucial in contexts where gradual and continuous change is required, such as in the biological growth of living organisms or geological processes. Generally, any noticeable change would take a long time to become apparent with these types of reactions.
Chemical Kinetics
Chemical kinetics is the field of chemistry that studies reaction rates and the factors that affect these rates. Understanding kinetics is essential because it explains how different conditions can influence the speed of reactions. Through kinetics, we can predict how changes in temperature, concentration, and the presence of catalysts or inhibitors might alter reaction rates. This field is fundamental in industries that require precise control over reaction speeds to optimize production or enhance safety.
Factors Affecting Reaction Rates
There are several factors that influence how fast or slow a reaction proceeds. Temperature is one primary factor; generally, increasing the temperature increases the reaction rate. Likewise, increasing the concentration of reactants typically speeds up a reaction. Pressure can also play a critical role in reactions involving gases. Additionally, catalysts enhance reaction rates by lowering the activation energy needed, while inhibitors slow down the rate of reaction. Understanding these factors allows chemists to control and manipulate reactions effectively to achieve desired outcomes.

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Most popular questions from this chapter

How does a catalyst influence the equilibrium constant?

One mole of \(\mathrm{PCl}_{5}\) is subjected to heating in a 1 1 vessel. The number of moles of \(\mathrm{PCl}_{3}\) formed at equilibrium is \(0.6 .\) Calculate the equilibrium constant for the dissociation of \(\mathrm{PCl}_{5}\).

Product the shift in equilibrium when the volume is decreased on the following equilibrium reactions: (i) \(\mathrm{Pcl}_{3(\mathrm{~g})}+\mathrm{Cl}_{2(\mathrm{~g})} \rightleftarrows \mathrm{PCl}_{5(\mathrm{~g})}\) (ii) \(\mathrm{N}_{2(g)}+\mathrm{O}_{2(\mathrm{~g})} \rightleftarrows 2 \mathrm{NO}_{(g)}\)

The value of equilibrium constant for a reversible reaction is \(3 \times 10^{-2}\). If the reaction quotient for the same reaction is \(5 \times 10^{-3}\), predict the direction of equilibrium reaction.

What is the effect of a catalyst on the equilibrium?
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