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Chapter 22: Problem 21

Briefly discuss the preparation and properties of carbon monoxide and carbon dioxide.

Short Answer

Expert verified
Carbon monoxide is prepared through partial oxidation of carbon containing compounds and is a strong reducing agent. Carbon dioxide is produced by burning fuels, respiration, and fermentation, and does not support combustion.

Step by step solution

01

Preparation and Properties of Carbon Monoxide

Carbon monoxide (CO) is prepared majorly in the industry through the partial oxidation of carbon containing compounds, mainly carbon. The process is typically carried out in a controlled environment, where a limited amount of oxygen is allowed to react with carbon to produce carbon monoxide. \n\nProperties: \n1. Carbon monoxide is a colorless, odorless, and tasteless gas, which makes it highly dangerous. \n2. It is less dense than air and slightly soluble in water.\n3. Carbon monoxide is a strong reducing agent and can reduce many metals from their oxides.
02

Preparation and Properties of Carbon Dioxide

Carbon dioxide (CO2) is produced in large quantities by burning fuels in air, as a product of respiration by living organisms, and fermentation processes.\n\nProperties: \n1. Carbon dioxide is a colorless and odorless gas.\n2. It is denser than air and soluble in water, forming carbonic acid.\n3. Under pressure, CO2 becomes a liquid, and under further pressure and cooling, it becomes a solid (dry ice). \n4. Carbon dioxide does not support combustion, unlike Oxygen.

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Most popular questions from this chapter

Consider the Frasch process. (a) How is it possible to heat water well above \(100^{\circ} \mathrm{C}\) without turning it into steam? (b) Why is water sent down the outermost pipe? (c) Why would excavating a mine and digging for sulfur be a dangerous procedure for obtaining the element?

Metal chlorides can be prepared in a number of ways: (a) direct combination of metal and molecular chlorine, (b) reaction between metal and hydrochloric acid, (c) acid-base neutralization, (d) metal carbonate treated with hydrochloric acid, (e) precipitation reaction. Give an example for each type of preparation.

Explain why nitric acid can be reduced but not oxidized.

Solid \(\mathrm{PCl}_{5}\) exists as \(\left[\mathrm{PCl}_{4}^{+}\right]\left[\mathrm{PCl}_{6}^{-}\right] .\) Draw Lewis structures for these ions. Describe the hybridization state of the \(\mathrm{P}\) atoms.

Lubricants used in watches usually consist of longchain hydrocarbons. Oxidation by air forms solid polymers that eventually destroy the effectiveness of the lubricants. It is believed that one of the initial steps in the oxidation is removal of a hydrogen atom (hydrogen abstraction). By replacing the hydrogen atoms at reactive sites with deuterium atoms, it is possible to substantially slow the overall oxidation rate. Why? (Hint: Consider the kinetic isotope effect.)
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