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Chapter 4: Problem 35

Give an example of a combination redox reaction, a decomposition redox reaction, and a displacement redox reaction.

Short Answer

Expert verified
A combination redox reaction example is \(2H_2 + O_2 \rightarrow 2H_2O\). A decomposition redox reaction example is \(2H_2O \rightarrow 2H_2 + O_2\). A displacement redox reaction example is \(CuSO4 + Zn \rightarrow Cu + ZnSO4\).

Step by step solution

01

Example of a Combination Redox Reaction

An example of a combination redox reaction is the formation of water through the combination of hydrogen and oxygen: \(2H_2 + O_2 \rightarrow 2H_2O\). In this scenario, hydrogen is oxidized (loses electrons) and oxygen is reduced (gains electrons).
02

Example of a Decomposition Redox Reaction

An example of a decomposition redox reaction is the breaking down of water into hydrogen and oxygen: \(2H_2O \rightarrow 2H_2 + O_2\). In this reaction, water is broken down into its component elements. Hydrogen is reduced (gains electrons) and oxygen is oxidized (loses electrons).
03

Example of a Displacement Redox Reaction

An example of a displacement redox reaction is the reaction between copper sulfate and zinc: \(CuSO4 + Zn \rightarrow Cu + ZnSO4\). In this reaction, Zinc displaces the copper from copper sulfate, resulting in the production of zinc sulfate and copper. Zinc is oxidized as it loses electrons and copper is reduced as it gains electrons.

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Most popular questions from this chapter

The following "cycle of copper" experiment is performed in some general chemistry laboratories. The series of reactions starts with copper and ends with metallic copper. The steps are as follows: (1) A piece of copper wire of known mass is allowed to react with concentrated nitric acid [the products are copper(II) nitrate, nitrogen dioxide, and water]. (2) The copper(II) nitrate is treated with a sodium hydroxide solution to form copper(II) hydroxide precipitate. (3) On heating, copper(II) hydroxide decomposes to yield copper(II) oxide. (4) The copper(II) oxide is reacted with concentrated sulfuric acid to yield copper(II) sulfate. (5) Copper(II) sulfate is treated with an excess of zinc metal to form metallic copper. (6) The remaining zinc metal is removed by treatment with hydrochloric acid, and metallic copper is filtered, dried, and weighed. (a) Write a balanced equation for each step and classify the reactions. (b) Assuming that a student started with \(65.6 \mathrm{~g}\) of copper, calculate the theoretical yield at each step. (c) Considering the nature of the steps, comment on why it is possible to recover most of the copper used at the start.

What volume of \(0.416 M \mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}\) should be added to \(255 \mathrm{~mL}\) of \(0.102 \mathrm{M} \mathrm{KNO}_{3}\) to produce a solution with a concentration of \(0.278 M \mathrm{NO}_{3}^{-}\) ions? Assume volumes are additive.

Phosphoric acid \(\left(\mathrm{H}_{3} \mathrm{PO}_{4}\right)\) is an important industrial chemical used in fertilizers, in detergents, and in the food industry. It is produced by two different methods. In the electric furnace method, elemental phosphorus \(\left(\mathrm{P}_{4}\right)\) is burned in air to form \(\mathrm{P}_{4} \mathrm{O}_{10},\) which is then reacted with water to give \(\mathrm{H}_{3} \mathrm{PO}_{4} .\) In the wet process, the mineral phosphate rock fluorapatite \(\left[\mathrm{Ca}_{5}\left(\mathrm{PO}_{4}\right)_{3} \mathrm{~F}\right]\) is reacted with sulfuric acid to give \(\mathrm{H}_{3} \mathrm{PO}_{4}\) (and \(\mathrm{HF}\) and \(\mathrm{CaSO}_{4}\) ). Write equations for these processes and classify each step as precipitation, acid-base, or redox reaction.

Distilled water must be used in the gravimetric analysis of chlorides. Why?

Sulfites (compounds containing the \(\mathrm{SO}_{3}^{2-}\) ions) are used as preservatives in dried fruits and vegetables and in wine making. In an experiment to test the presence of sulfite in fruit, a student first soaked several dried apricots in water overnight and then filtered the solution to remove all solid particles. She then treated the solution with hydrogen peroxide \(\left(\mathrm{H}_{2} \mathrm{O}_{2}\right)\) to oxidize the sulfite ions to sulfate ions. Finally, the sulfate ions were precipitated by treating the solution with a few drops of a barium chloride \(\left(\mathrm{BaCl}_{2}\right)\) solution. Write a balanced equation for each of the preceding steps.
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