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The document covers the fundamentals of stoichiometry of hydrocarbon combustion, focusing on chemical reactions, concentrations, and combustion of hydrocarbons. Key topics include:
2/17/2023
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This page discusses two important ratios used in combustion analysis, particularly in aviation:
Vocabulary:
- AFR (Air/Fuel Ratio): The ratio of air mass-flow to fuel mass-flow
- FAR (Fuel/Air Ratio): The ratio of fuel mass-flow to air mass-flow
These ratios are essential for analyzing and optimizing combustion processes in various applications, especially in aircraft engines.
This section delves into the principles of chemical reactions and stoichiometry. It uses a simple example to illustrate how species react in exact proportions.
Example: In the reaction A + 2B → C, 1 mole of A reacts with 2 moles of B to produce 1 mole of C.
Definition: Stoichiometry in chemical reactions refers to the exact proportions in which species react.
The page emphasizes the importance of understanding these proportions in chemical reactions, which is crucial for chemical reaction stoichiometry basics.
The final page begins an example calculation for determining the stoichiometric air required for methane (CH₄) combustion. This practical application demonstrates how to apply the principles of stoichiometry of hydrocarbon combustion to a real-world problem.
This section examines the combustion of a lean methane mixture in air, assuming a 5% air excess. The balanced equation for this reaction is:
CH₄ + 2.1O₂ + 7.9N₂ → CO₂ + 2H₂O + 7.9N₂ + 0.1O₂
Highlight: In a lean mixture combustion, there is excess oxygen present in the flue gas.
This example illustrates how the presence of excess air affects the combustion reaction and the resulting flue gas composition.
This page analyzes the composition of flue gas resulting from the stoichiometric combustion of methane in air. It calculates the concentrations of CO₂, H₂O, and N₂ in the flue gas based on the number of moles of each component.
Example: In the flue gas, the concentrations are:
- 9.5% CO₂
- 19% H₂O
- 71.5% N₂
These calculations demonstrate how to determine the composition of combustion products using stoichiometric principles.
This page discusses the various types of oxidizers used in combustion processes. The four main types of oxidizers covered are:
Understanding the different types of oxidizers is crucial for analyzing and optimizing combustion processes in various applications.
This section introduces the concept of stoichiometric air, which is the theoretical minimum amount of air required for complete combustion of a fuel.
Definition: Stoichiometric air is the minimum air required in a stoichiometric mixture, as determined by the equation of stoichiometry for the oxygen/fuel reaction.
The page explains that the actual combustion air depends on the assumed air excess, which is expressed using the equivalence ratio or stoichiometric ratio.
This page introduces the basic concepts of stoichiometry and chemical reactions. It covers the definitions of atomic unit mass, moles, and kilomoles, which are fundamental to understanding chemical reaction stoichiometry basics.
Definition: A mole is defined as 6.022 x 10^23 atoms, which is known as Avogadro's number.
Highlight: The volume of 1 mole of a perfect gas at 0°C and 1 atm pressure is 22.4141 liters.
The page also explains that the mass of one mole (or kilomole) is equal to the relative atomic mass in grams (or kilograms).
This page categorizes fuel mixtures into three types based on their composition relative to the stoichiometric ratio:
Understanding these mixture types is crucial for optimizing combustion processes and controlling emissions in various applications.
This page discusses how to express the amounts of different species in a mixture. It introduces three important concepts:
Vocabulary:
- Concentration: The amount of a species per unit volume
- Mole fraction: The number of moles of a species divided by the total number of moles of all species
- Mass fraction: The mass of a species divided by the total mass of all species
These concepts are essential for understanding and calculating the composition of mixtures in stoichiometry of hydrocarbon combustion.
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Jay Gale
@jaygale_mnxt
·
1 Follower
Follow
The document covers the fundamentals of stoichiometry of hydrocarbon combustion, focusing on chemical reactions, concentrations, and combustion of hydrocarbons. Key topics include:
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This page discusses two important ratios used in combustion analysis, particularly in aviation:
Vocabulary:
- AFR (Air/Fuel Ratio): The ratio of air mass-flow to fuel mass-flow
- FAR (Fuel/Air Ratio): The ratio of fuel mass-flow to air mass-flow
These ratios are essential for analyzing and optimizing combustion processes in various applications, especially in aircraft engines.
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Improve your grades
Join milions of students
By signing up you accept Terms of Service and Privacy Policy
This section delves into the principles of chemical reactions and stoichiometry. It uses a simple example to illustrate how species react in exact proportions.
Example: In the reaction A + 2B → C, 1 mole of A reacts with 2 moles of B to produce 1 mole of C.
Definition: Stoichiometry in chemical reactions refers to the exact proportions in which species react.
The page emphasizes the importance of understanding these proportions in chemical reactions, which is crucial for chemical reaction stoichiometry basics.
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Improve your grades
Join milions of students
By signing up you accept Terms of Service and Privacy Policy
The final page begins an example calculation for determining the stoichiometric air required for methane (CH₄) combustion. This practical application demonstrates how to apply the principles of stoichiometry of hydrocarbon combustion to a real-world problem.
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Join milions of students
By signing up you accept Terms of Service and Privacy Policy
This section examines the combustion of a lean methane mixture in air, assuming a 5% air excess. The balanced equation for this reaction is:
CH₄ + 2.1O₂ + 7.9N₂ → CO₂ + 2H₂O + 7.9N₂ + 0.1O₂
Highlight: In a lean mixture combustion, there is excess oxygen present in the flue gas.
This example illustrates how the presence of excess air affects the combustion reaction and the resulting flue gas composition.
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Improve your grades
Join milions of students
By signing up you accept Terms of Service and Privacy Policy
This page analyzes the composition of flue gas resulting from the stoichiometric combustion of methane in air. It calculates the concentrations of CO₂, H₂O, and N₂ in the flue gas based on the number of moles of each component.
Example: In the flue gas, the concentrations are:
- 9.5% CO₂
- 19% H₂O
- 71.5% N₂
These calculations demonstrate how to determine the composition of combustion products using stoichiometric principles.
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Improve your grades
Join milions of students
By signing up you accept Terms of Service and Privacy Policy
This page discusses the various types of oxidizers used in combustion processes. The four main types of oxidizers covered are:
Understanding the different types of oxidizers is crucial for analyzing and optimizing combustion processes in various applications.
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Improve your grades
Join milions of students
By signing up you accept Terms of Service and Privacy Policy
This section introduces the concept of stoichiometric air, which is the theoretical minimum amount of air required for complete combustion of a fuel.
Definition: Stoichiometric air is the minimum air required in a stoichiometric mixture, as determined by the equation of stoichiometry for the oxygen/fuel reaction.
The page explains that the actual combustion air depends on the assumed air excess, which is expressed using the equivalence ratio or stoichiometric ratio.
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Improve your grades
Join milions of students
By signing up you accept Terms of Service and Privacy Policy
This page introduces the basic concepts of stoichiometry and chemical reactions. It covers the definitions of atomic unit mass, moles, and kilomoles, which are fundamental to understanding chemical reaction stoichiometry basics.
Definition: A mole is defined as 6.022 x 10^23 atoms, which is known as Avogadro's number.
Highlight: The volume of 1 mole of a perfect gas at 0°C and 1 atm pressure is 22.4141 liters.
The page also explains that the mass of one mole (or kilomole) is equal to the relative atomic mass in grams (or kilograms).
Access to all documents
Improve your grades
Join milions of students
By signing up you accept Terms of Service and Privacy Policy
This page categorizes fuel mixtures into three types based on their composition relative to the stoichiometric ratio:
Understanding these mixture types is crucial for optimizing combustion processes and controlling emissions in various applications.
Access to all documents
Improve your grades
Join milions of students
By signing up you accept Terms of Service and Privacy Policy
This page discusses how to express the amounts of different species in a mixture. It introduces three important concepts:
Vocabulary:
- Concentration: The amount of a species per unit volume
- Mole fraction: The number of moles of a species divided by the total number of moles of all species
- Mass fraction: The mass of a species divided by the total mass of all species
These concepts are essential for understanding and calculating the composition of mixtures in stoichiometry of hydrocarbon combustion.
Average App Rating
Students use Knowunity
In Education App Charts in 12 Countries
Students uploaded study notes
iOS User
Stefan S, iOS User
SuSSan, iOS User
