Using redox reactions

Galvanic cells use redox reactions to generate electrical current. Electrical current can also drive redox reactions, and the same stoichiometric relationships apply to such processes, as we describe in Section 19-1. 

This reaction occurs on the surface of the zinc strip, where electrons are transferred from zinc atoms to copper(II) ions when these atoms and ions are in direct contact. A common technological invention called a galvanic cell uses redox reactions, such as the one described above, to release energy in the form of electricity. 

Scheme 1.1 Methods to increase H-bond strength using redox reactions.

Some organisms use redox reactions to produce light, which they use in communication. This light production is called bioluminescence. 

Battery A device that has two or more voltaic cells connected together. The term is also used to describe any device that converts chemical energy into electrical energy using redox reactions. 

Oxidation-reduction (electron transfer) reactions are important in chemistry and biology. When a chemical oxidation of A by B occurs, B itself is reduced - an electron transfer process has occurred. For such chemical processes, there is always a partnership between an oxidant (which is reduced in carrying out its task) and a reductant (which is oxidized in the reaction) thus we frequently talk of oxidation-reduction, or (for ease of use) redox, reactions for what are essentially electron transfer processes. Of course, an electron can be... 

When the modifier is a base metal, the most commonly used redox reaction is catalytic reduction. Nevertheless, the refilling method with preadsorbed hydro-... 

Danes (4 4) reported on an ILM using a carrier molecule as an electron carrier. This allows one to use redox reactions to transport charge as well as mass. 

Bleaches use redox reactions to remove color from material (see Chapter 9 for a discussion of redox reactions). Most bleaches are oxidizing scents. The most common bleach used in the home is a 5 percent solution of sodium hypochlorite. This type of bleach is produced by bubbling chlorine gas through a sodium hydroxide solution ... 

We have observed that voltaic cells use redox reactions that proceed spontaneously. Any reaction that can occur in a voltaic cell to produce a positive emf must be spontaneous. Consequently, it is possible to decide whether a redox reaction will be spontaneous by using half-cell potentials to calculate the emf associated with it. 

Oxidation and Reduction Redox reactions are common in nature, in industry, and in many everyday processes. Batteries use redox reactions to generate electrical current. Our bodies use redox reactions to obtain energy from glucose. In addition, the bleaching of hair, the rusting of iron, and the electroplating of metals all involve redox reactions. 

Galvanic cells use redox reactions to produce electricity. These cells are commonly Ccdled batteries, but sometimes this name is somewhat incorrect, because a battery is composed of two or more cells connected together. You put a battery in your car, but you put a cell into your flashlight. 

Electronic properties can be studied by photoelectrochemistry using redox reactions at passivated metal surfaces in the dark or with illumination. Their knowledge is very valuable to understand layer formation and corrosion phenomena for open circuit conditions, i.e., under the influence of redox systems within the electrolyte. Furthermore layer formation includes often oxidation of intermediates, i.e., oxidation of lower valent to higher valent cations, which requires electronic conduction through the already existing film. Similarly layer reduction needs electron transfer across the film. 

A variation on the theme is the fuel cell , a device first constructed by Sir William Grove (1811-1896) in 1840 on the basis of ideas proposed by the German chemist Christian Schonbein (1799 -1868) shortly before. A fuel cell works in much the same way as the cells I have already described, using redox reactions to generate a flow of electrons. However instead of the reagents being sealed in at manufacture they are supplied continuously from an external source, like fuel to a furnace, as the reaction proceeds. 

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