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Chapter 17: Problem 1

Give some examples of how we make good use of oxidation-reduction reactions in everyday life.

Short Answer

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Oxidation-reduction reactions, also known as redox reactions, are essential in everyday life. Some examples include: 1) Batteries, which rely on redox reactions to generate electricity; 2) Combustion, where fuels like gasoline react with oxygen to release heat and light energy; 3) Rusting of iron, a slow redox reaction between iron, oxygen, and water; 4) Photosynthesis, a redox reaction in plants converting light energy into chemical energy; and 5) Human metabolism, where redox reactions like cellular respiration help break down nutrients to release energy for our cells.

Step by step solution

01

Example 1: Batteries

Batteries, which are commonly used in everyday life for powering electronic devices, rely on redox reactions to generate electricity. In a simple battery, there are two electrodes (cathode and anode) that are made of different materials. When connected to a closed circuit, a redox reaction occurs between the two electrodes, causing electrons to flow from the anode to the cathode. This flow of electrons provides electric current to power devices.
02

Example 2: Combustion

Combustion is another example of oxidation-reduction reactions that we commonly encounter in everyday life. In combustion reactions, a fuel (like gasoline, coal, or natural gas) reacts with oxygen, which results in the release of energy in the form of heat and light. The process of burning a candle, using a gas stove or driving a car all involve combustion reactions and the transfer of electrons between the fuel and oxygen.
03

Example 3: Rusting of Iron

The rusting of iron is a slow oxidation-reduction reaction that occurs over time when iron is exposed to oxygen and water. During this process, iron loses electrons and oxygen gains electrons. The rust (iron oxide) that forms on the surface of the iron is the product of this redox reaction. This is an example of a negative impact of redox reactions on everyday life, as it leads to the deterioration of iron and steel structures.
04

Example 4: Photosynthesis

Photosynthesis, a vital process for maintaining life on Earth, is an example of a redox reaction that occurs in plants. In this reaction, water molecules are oxidized (losing electrons) and carbon dioxide molecules are reduced (gaining electrons). This process converts light energy into chemical energy, which is used to synthesize glucose and oxygen - the substances necessary for plant growth and the release of oxygen into the atmosphere for other living organisms to breathe.
05

Example 5: Human metabolism

Our own bodies use redox reactions as a vital part of metabolism. When we consume food, our body breaks down nutrients, such as carbohydrates, fats, or proteins, in order to release the energy stored in their chemical bonds. One important redox reaction that occurs in our cells is cellular respiration. In this process, glucose and other molecules are broken down with the help of oxygen, releasing energy that our cells need to function properly. In conclusion, oxidation-reduction reactions play a crucial role in a wide range of processes and activities in everyday life. From powering electronic devices to maintaining the balance of life on Earth, these reactions are an essential component of our world.

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Most popular questions from this chapter

How is an oxidation-reduction reaction set up as a galvanic cell (battery)? How is the transfer of electrons between reducing agent and oxidizing agent made useful?

Although aluminum is one of the most abundant metals on the earth, most people make an effort to recycle aluminum cans. How might this be related to the process by which aluminum metal is produced?

What process is represented by the corrosion of a metal? Why is corrosion undesirable?

What is a salt bridge? Why is a salt bridge necessary in a galvanic cell? Can some other method be used in place of the salt bridge?

Why does an alkaline dry cell battery typically last longer than a normal dry cell? Write the chemical equation for the overall cell reaction in an alkaline dry cell.
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