Question

give 10 examples of oxidation and reduction reaction​

Answer 1

Ten examples of oxidation and reduction reaction​:

1. $Fe(s) + CuSO4(aq)\rightarrow FeSO4(aq) + Cu(s)$

In this reaction, iron is oxidized, and copper is reduced.

2.$Zn(s)+2HCl(aq)\rightarrow ZnCl_{2} (aq)+H_{2}(g)$

In this reaction, zinc is oxidized, and hydrogen is reduced.

3.$CuO + H_{2} \rightarrow Cu +H_{2} O$

In this reaction, hydrogen is oxidized, and copper is reduced.

4.$3ClO^{-} (aq)\rightarrow ClO_{3}^{-} (aq)+2Cl^{-} (aq)$

In this reaction, chlorine is being oxidized as well as reduced.

5.$MnO4^{-} + I^{-} \rightarrow MnO_{2} + I_{2}$

In this reaction, iodine is oxidized, and manganese is reduced.

6.$2C_{8} H_{18}+25O_{2} \rightarrow 16 CO_{2} (g)+18H_{2}O$

In this reaction, carbon is oxidized, and oxygen is reduced.

7.$Pb + PbO_{2} + 2H_{2} SO_{4}\rightarrow 2PbSO_{4} + 2H_{2} O$

In this reaction, lead is being oxidized as well as reduced.

8.$H_{2} S + Cl_{2}\rightarrow 2HCl + S$

In this reaction, sulfur is oxidized, and chlorine is reduced.

9.$2Al(s) + Fe_{2} O_{3} (s)\rightarrow Al_{2} O_{3} (s) + 2Fe(l)$

In this reaction, aluminum is oxidized, and iron is  reduced.

10.$2K + MgCl_{2}\rightarrow 2KCl + Mg$

In this reaction, potassium is oxidized, and magnesium is reduced.

Answer 2

Answer:

We find examples of reducing oxidation or redox reactions almost every time we analyze reactions used as heat sources or function. When natural gas burns, for example, an oxidation reduction reaction occurs that releases more than 800 kJ / mol of energy.

CH4 (g) + 2 O2 (g) -----> CO2 (g) + 2 H2O (g)

In our bodies, the sequence of oxidation reactions is used to burn sugars, such as glucose (C6H12O6) and fatty acids in the fats we eat.

C6H12O6 (aq) + 6 O2 (g) -----> 6 CO2 (g) + 6 H2O (l)

CH3 (CH2) 16CO2H (aq) + 26 O2 (g) -----> 18 CO2 (g) + 18 H2O (l)

We do not need to limit ourselves to a reaction that can be used as a source of energy, however, in order to find examples of oxidation reduction reactions. Silver metal, for example, is oxidized when it comes in contact with a small amount of H2S or SO2 in the atmosphere or egg-like foods, rich in sulfur compounds.

4 Ag (ama) + 2 H2S (g) + O2 (g) -----> 2 Ag2S (ama) + 2 H2O (g)

Fortunately, the Ag2S film that accumulates in the metal surface creates a protective coating that reduces the additional oxidation of the silver metal.

Silver contamination is just one example of a broad-spectrum reduction of oxidation that falls under the general heading of corrosion. Another example is a series of reactions that occur when metal or metal rust. When burned, the metal combines with oxygen to form a mixture of iron (II) and iron (III) oxides.

2 Fe (ama) + O2 (g) -----> 2 FeO (ama)

2 Fe (these) + 3 O2 (g) -----> 2 Fe2O3 (ama)

The melted iron even mixes with water to form an aqueous solution of Fe2 + ion and H2 gas.

Fe (l) + 2 H2O (l) -----> Fe2 + (aq) + 2 OH- (aq) + H2 (g)

However, with room temperature, all three conditions are so slow that they are almost ignored.

Iron vene rust only at room temperature where there is both oxygen and water. In the course of this reaction, iron is released by oxid to provide a liquid form of iron (II) oxide.

2 Fe (these) + O2 (aq) + 2 H2O (l) -----> 2 FeO H2O (ama)

Because this compound has a solid formula like Fe (OH) 2, it is often mistakenly called iron (II), or ferrous, hydroxide. The FeO H2O formed in this reaction is then dissolved in water-soluble O2 to provide a liquid form of iron (III), or ferric, oxide.

4 FeO H2O (ama) + O2 (aq) + 2 H2O (l) -----> 2 Fe2O3 3 H2O (ama)

To further complicate matters, FeO H2O built into the metal mixes with Fe2O3 3 H2O to provide a liquid form of iron oxide (Fe3O4).

FeO H2O (ama) + Fe2O3 -----> 3 H2O (ama) Fe3O4 n H2O (ama)

Because this reaction occurs only when there is both water and oxygen, cars often rust where water collects. In addition, because the simplest way to prevent corrosion is to cover the metal so that it does not come in contact with water, initially cars were painted for one reason only - to delay corrosion.

#SPJ2