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What is incomplete combustion of fossil fuels? Why can this be a problem?

Short Answer

Expert verified
Incomplete combustion of fossil fuels occurs when there is insufficient oxygen supply for a substance to burn completely, leading to the production of carbon monoxide (CO) and partially oxidized hydrocarbons (like soot or smoke). This can be problematic because it results in the emission of toxic carbon monoxide gas, release of harmful particulate matter, and lower energy efficiency, all of which negatively impact human health and the environment.

Step by step solution

01

Definition of Fossil Fuels and Combustion

Fossil fuels are energy sources derived from organic matter formed millions of years ago. They include coal, oil, and natural gas. They are widely used as primary energy sources due to their high energy content. Combustion is a chemical reaction in which a substance reacts with oxygen, usually producing heat and light energy in the form of fire.
02

Incomplete Combustion

Incomplete combustion occurs when there is insufficient oxygen supply for a substance (in this case, a fossil fuel) to burn completely. In such a scenario, instead of producing carbon dioxide (CO2) and water (H2O) as the primary products, the substance produces carbon monoxide (CO) and partially oxidized hydrocarbons (like soot or smoke).
03

Problems Caused by Incomplete Combustion

Incomplete combustion of fossil fuels can lead to several problems, such as: 1. Carbon monoxide (CO) emission: Carbon monoxide is a toxic gas that is odorless and colorless, making it difficult to detect. CO competes with oxygen in hemoglobin, leading to oxygen deprivation in the body, which can cause serious health issues and even death. 2. Particulate matter (smoke and soot): Incomplete combustion releases fine particles (particulate matter) into the air. These particles can cause respiratory problems, lung damage, and other health issues. They also contribute to air pollution and reduced visibility. 3. Lower energy efficiency: Incomplete combustion leads to a lower energy output compared to complete combustion. As a result, more fuel must be burned to obtain the same amount of energy, which negatively impacts fuel efficiency and overall energy consumption. In conclusion, incomplete combustion of fossil fuels not only wastes valuable resources but also leads to hazardous emissions that pose significant risks to human health and the environment.

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Most popular questions from this chapter

A biology experiment requires the preparation of a water bath at \(37.0^{\circ} \mathrm{C}\) (body temperature). The temperature of the cold tap water is \(22.0^{\circ} \mathrm{C},\) and the temperature of the hot tap water is \(55.0^{\circ} \mathrm{C} .\) If a student starts with 90.0 \(\mathrm{g}\) cold water, what mass of hot water must be added to reach \(37.0^{\circ} \mathrm{C} ?\)

A system undergoes a process consisting of the following two steps: Step 1: The system absorbs 72 \(\mathrm{J}\) of heat while 35 \(\mathrm{J}\) of work is done on it. Step \(2 :\) The system absorbs 35 \(\mathrm{J}\) of heat while performing 72 \(\mathrm{J}\) of work. Calculate \(\Delta E\) for the overall process.

For the following reactions at constant pressure, predict if \(\Delta H>\Delta E, \Delta H<\Delta E,\) or \(\Delta H=\Delta E .\) a. \(2 \mathrm{HF}(g) \longrightarrow \mathrm{H}_{2}(g)+\mathrm{F}_{2}(g)\) b. \(\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \longrightarrow 2 \mathrm{NH}_{3}(g)\) c. \(4 \mathrm{NH}_{3}(g)+5 \mathrm{O}_{2}(g) \longrightarrow 4 \mathrm{NO}(g)+6 \mathrm{H}_{2} \mathrm{O}(g)\)

A system absorbs 35 \(\mathrm{J}\) of heat and has 25 \(\mathrm{J}\) of work performed on it. The system then returns to its initial state by a second step. If 5 \(\mathrm{J}\) of heat are given off in the second step, how much work is done by the system in the second step?

The preparation of \(\mathrm{NO}_{2}(g)\) from \(\mathrm{N}_{2}(g)\) and \(\mathrm{O}_{2}(g)\) is an endothermic reaction: $$ \mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{NO}_{2}(g)(\text { unbalanced }) $$ The enthalpy change of reaction for the balanced equation (with lowest whole- number coefficients) is \(\Delta H=67.7 \mathrm{kJ}\) . If \(2.50 \times 10^{2} \mathrm{mL} \mathrm{N}_{2}(g)\) at \(100 .^{\circ} \mathrm{C}\) and 3.50 atm and \(4.50 \times\) \(10^{2} \mathrm{mL} \mathrm{O}_{2}(g)\) at \(100 .^{\circ} \mathrm{C}\) and 3.50 atm are mixed, what amount of heat is necessary to synthesize the maximum yield of \(\mathrm{NO}_{2}(g) ?\)

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