Combustion Senatorlibya
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The document discusses the combustion stoichiometry of benzene (C6H6) as a fuel. It defines the complete combustion reaction of benzene with air and calculates the stoichiometric air to fuel ratio. It also discusses fuel lean and fuel rich mixtures, showing how the composition of combustion products varies with excess or insufficient air. Plots are included showing how nitrogen content, carbon dioxide content, and dew point temperature change with air to fuel ratio.
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The document summarizes the fuel supply systems of SI (spark ignition) and CI (compression ignition) engines. For SI engines, the key components are the fuel tank, fuel pump, fuel filter, carburetor and inlet manifold. For CI engines, the key components are the fuel tank, fuel transfer pump, fuel filter, injection pump and injection nozzles. The fuel transfer pump moves fuel through the fuel filter to the injection pump. The injection pump then supplies precise, high-pressure fuel to the injection nozzles for injection into each cylinder at the correct time.
Chapter 03-Combustion Processes
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The document discusses different types of chemical bonding including ionic bonding, covalent bonding, and dative covalent bonding. Ionic bonding involves electron transfer between metals and nonmetals to form ionic compounds with electrostatic attraction between cations and anions. Covalent bonding involves sharing of electron pairs between atoms. Sigma and pi bonds are discussed as well as dot-and-cross diagrams and Lewis structures. Dative covalent bonding occurs when both electrons in a covalent bond come from the same atom, such as in a coordinate bond where a donor atom provides both electrons.
Chemical Reaction
The document discusses different types of chemical reactions:
1) Decomposition reactions involve a single compound breaking down into simpler substances. An example is calcium carbonate decomposing to calcium oxide and carbon dioxide.
2) Combination reactions involve two substances combining to form a new compound. An example is calcium oxide and sulfur dioxide combining to form calcium sulfite.
3) Single replacement reactions involve an element replacing another in a compound. An example is copper displacing silver from silver nitrate.
4) Double replacement reactions involve ion exchange between two compounds in solution and forming a precipitate. An example is silver nitrate and sodium chloride forming silver chloride and sodium nitrate precipitates.
5) Combustion reactions
Ch. 3 stoichiometry
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The document discusses the fundamentals of biomass combustion, including the processes of drying, pyrolysis, flaming combustion, and glowing combustion. It also covers combustion equipment designs like inclined grate furnaces, spreader stokers, cyclonic and suspension fired systems, and fluidized bed combustion. The goal of combustion system design is to efficiently oxidize the biomass through sufficient mixing of the fuel with oxygen and controlling residence times and temperatures.
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Unit 4 introduction to fuels and combustion
This document provides an overview of fuels and combustion. It defines fuels as either natural/primary sources (solid, liquid, gas) or manufactured sources (solid, liquid, gas). Good fuels are characterized by high calorific value, moderate ignition temperature, low moisture/ash content, and being low cost and easy to store/transport. Calorific value measures the total heat released from combusting a unit of fuel, and can be expressed in various units for solids, liquids and gases. Higher calorific value refers to heat released when products cool to room temperature, while lower calorific value excludes heat of vaporization of water formed. Calorific value is determined experimentally by combusting a known fuel amount and
Chapter 14
The document discusses emerging fire protection technologies including building information modeling platforms that allow data sharing, computer fire modeling to understand fire spread, and performance-based design approaches. New detection methods like video cameras and gas/particulate analysis are presented. Mass notification, multipurpose piping systems, variable speed fire pumps, compressed air foam systems, and aerosol suppression systems are emerging technologies aimed to improve fire detection, control, and suppression.
Stoichiometric Calculations
This is an Excerpt from www.cabrillo.edu.
There was no better way to put it according to me. So I am sharing this file as a part of a good study.
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The presentation is discussing
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ppt of fuel and combustion
This document is a presentation by Group 4 of Diploma Civil "A" on the topic of fuel and combustion. It introduces different types of fuels such as solid, liquid, and gaseous fuels. Solid fuels discussed include coal, coke, and charcoal. Liquid fuels mentioned are tar, kerosene, diesel, petrol, and gas. Gaseous fuels include natural gas, coal gas, and biogas. The presentation covers the characteristics of good fuels, classification of fuels, advantages and disadvantages of different fuel types, and concepts of combustion and calorific values. In the end, the group thanks their professor Mr. Tarang Agarwal for giving them the opportunity to present.
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Module 8 (fuels and combustion)
This document discusses fuels and combustion. It defines a fuel as a substance that undergoes rapid chemical union with oxygen to produce combustion. Combustion is the rapid oxidation of an element that liberates heat. There are four main types of fuel: solid, liquid, gaseous, and nuclear. The main combustible elements are carbon, hydrogen, and sulfur. Hydrocarbons are the main components of fuels and can be paraffins, olefins, aromatics, or alcohols. Complete combustion occurs when all combustible elements are fully oxidized, while incomplete combustion occurs when some elements are not fully oxidized. Air is needed for combustion and is composed of oxygen and nitrogen. Theoretical air is the
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This document summarizes key concepts in stoichiometry including:
1) Chemical equations represent chemical reactions and show reactants on the left and products on the right. Coefficients are used to balance equations.
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A company has a cogeneration power plant and a conventional heater to meet its electricity and heat demands. The cogeneration plant has an electrical efficiency of 30%, a heat to power ratio of 2, and can be adjusted to meet the heat demand. The question asks to determine the optimal configuration to minimize fuel consumption as the heat demand varies from 1 to 6 MW.
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Thermochemical study of Energy associated with reactions using python.
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Hess's law states that the total enthalpy change for a reaction is independent of the pathway between the initial and final states. To calculate the enthalpy change of a reaction, standard enthalpy change values can be used for the elementary steps that add up to the overall reaction through algebraic manipulation. For the reaction of 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g), using standard enthalpy change values for the elementary steps gives an overall exothermic enthalpy change of -906.3 kJ.
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Hess's law states that the total enthalpy change for a reaction is independent of the pathway between the initial and final states. To calculate the enthalpy change of a reaction, standard enthalpy change values can be used and the coefficients must be treated accordingly when combining multiple reactions to arrive at the desired overall reaction. The enthalpy change is then calculated by taking the algebraic sum of the individual reaction enthalpies.
AP Chemistry Chapter 3 Outline
This document summarizes key concepts in stoichiometry including:
1) Chemical equations represent chemical reactions and include reactants, products, and coefficients to balance the equation.
2) Reaction types include combination, decomposition, and combustion reactions.
3) Formula weights, molecular weights, moles, molar mass, and limiting reactants are important concepts for solving stoichiometry problems quantitatively.
4) Empirical formulas can be calculated from elemental composition data using mole ratios.
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This document summarizes key concepts in stoichiometry including:
1) Chemical equations represent chemical reactions and include reactants, products, and coefficients to balance the equation.
2) Reaction types include combination, decomposition, and combustion reactions.
3) Formula weights, molecular weights, moles, molar mass, and limiting reactants are important concepts for solving stoichiometry problems quantitatively.
4) Empirical formulas can be calculated from elemental composition data using mole ratios.
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#23 Key
1. Calculate the enthalpy change for the reaction P4O6 (s) + 2 O2 (g) → P4O10 (s) using given enthalpy values for related reactions.
2. Calculate the standard enthalpy of reaction (ΔH°) for several reactions using standard enthalpies of formation from appendix C.
3. Calculate the standard enthalpy of formation of gaseous diborane (B2H6) using thermochemical cycles and given reaction enthalpies.
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1. The document contains a practice test with multiple choice questions about chemical kinetics and equilibrium.
2. Questions cover topics like reaction rates, rate laws, reaction orders, equilibrium constants, Le Chatelier's principle, and the Haber process.
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Module 7 - Energy Balance chemical process calculations
Chemical process calculations involve various computations and analyses to design, optimize, and understand chemical processes. Here are some descriptions highlighting different aspects of chemical process calculations:
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Material balances are the cornerstone of chemical process calculations, ensuring that the amounts of all components entering and leaving a system are properly accounted for.
These calculations involve tracking the flow rates and compositions of substances throughout a process, often using mass or mole balances.
Energy Balances:
Energy balances involve quantifying the energy inputs and outputs in a chemical process.
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Reaction Kinetics:
Chemical reactions kinetics calculations focus on understanding the rates at which reactions occur and how they are influenced by various factors such as temperature, pressure, and catalysts.
These calculations help in determining the optimal reaction conditions and designing reactors for desired conversion rates.
Phase Equilibrium Calculations:
Phase equilibrium calculations deal with determining the distribution of components between different phases in a system, such as liquid-liquid or vapor-liquid equilibrium.
These calculations are essential for designing separation processes like distillation, extraction, and absorption.
Thermodynamic Calculations:
Thermodynamic calculations involve applying thermodynamic principles to predict the behavior of chemical systems.
These calculations include determining properties such as enthalpy, entropy, Gibbs free energy, and fugacity, which are crucial for process design and optimization.
Process Simulation:
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Combustion Senatorlibya
- 1. The Theory of Combustion Benzene as a Fuel
- 3. Combustion Stoichiometry Air contains molecular nitrogen N 2 , when the products are low temperature the nitrogen is not significantly affected by the reaction, it is considered inert . The complete reaction of a general hydrocarbon C H with air is: The above equation defines the stoichiometric proportions of fuel and air. Example: For benzene (C 3 H 8 ) = 6 and = 6 C balance: = b H balance: = 2c c = / 2 O balance: 2a = 2b + c a = b + c / 2 a = + /4 N balance: 2 ( 3.76)a = 2d d = 3.76a/2 d = 3.76( + / 4 ) C 6 H 6 + (7.5)(O 2 +3.76N 2 ) 6CO 2 +3H 2 O+3.76(7.5)N 2
- 4. Combustion Stoichiometry Note above equation only applies to stoichiometric mixture For benzene (C 6 H 6 ), (A/F) s = 13.2 The stoichiometric mass based air/fuel ratio for C H fuel is: The products of benzene: 6CO 2 +3H 2 O+3.76(7.5)N 2 =6 + 3 + 3.76x7.5 = 37.2 mol N 2 (%)=75.81% H 2 O(%)=8.1% CO 2 (%)=16.13%
- 12. Plotting >> dewpoint1=[58.53 54.666 47.087]; >> dewpoint2=[74.5 70.77 61.765]; >> dewpoint3=[84.431 80.5 71]; >> plot(afr,dewpoint1) >> hold on >> plot(afr,dewpoint2) >> hold on >> plot(afr,dewpoint3) >> grid