Calorific Value(Heat of combustion): Difference between revisions
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==Main Idea== | ==Main Idea== | ||
The Calorific Value of a sample, also known as its Heat of Combustion, is defined as the amount of heat released during the combustion. For combustion to occur, a hydrocarbon is typically put into contact with oxygen and supplied the necessary activation energy. Once the reaction occurs, carbon dioxide, water, and heat are the products. This heat is usually enough to continue the reaction, allowing a flammable substance to burn until there is none left. | The Calorific Value of a sample, also known as its Heat of Combustion, is defined as the amount of heat released during the complete combustion of the sample. For combustion to occur, a hydrocarbon is typically put into contact with oxygen and supplied the necessary activation energy. Once the reaction occurs, carbon dioxide, water, and heat are the products. This newfound heat is usually enough to continue the reaction, allowing a flammable substance to burn until there is none left. | ||
The Heat of Combustion is typically measured | The Heat of Combustion is typically measured through experiments using a bomb calorimeter, where the sample is supplied with excess oxygen. This device measures the temperature change. From this, the Heat of Combustion can be computed using the [[Thermal Energy| Thermal Energy Equation]]. | ||
===Mathematical Model=== | ===Mathematical Model=== | ||
A typical combustion reaction looks like this: | |||
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==References== | ==References== | ||
https://en.wikipedia.org/wiki/Heat_of_combustion <br> | |||
https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Book%3A_Introductory_Chemistry_(CK-12)/17%3A_Thermochemistry/17.14%3A_Heat_of_Combustion <br> | |||
https://www.ck12.org/chemistry/heat-of-combustion/lesson/Heat-of-Combustion-CHEM/ <br> | |||
Revision as of 09:26, 2 August 2019
Main Idea
The Calorific Value of a sample, also known as its Heat of Combustion, is defined as the amount of heat released during the complete combustion of the sample. For combustion to occur, a hydrocarbon is typically put into contact with oxygen and supplied the necessary activation energy. Once the reaction occurs, carbon dioxide, water, and heat are the products. This newfound heat is usually enough to continue the reaction, allowing a flammable substance to burn until there is none left.
The Heat of Combustion is typically measured through experiments using a bomb calorimeter, where the sample is supplied with excess oxygen. This device measures the temperature change. From this, the Heat of Combustion can be computed using the Thermal Energy Equation.
Mathematical Model
A typical combustion reaction looks like this:
Computational Model
Examples
Simple
Middling
Difficult
Connectedness
History
See also
Further reading
External links
References
https://en.wikipedia.org/wiki/Heat_of_combustion
https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Book%3A_Introductory_Chemistry_(CK-12)/17%3A_Thermochemistry/17.14%3A_Heat_of_Combustion
https://www.ck12.org/chemistry/heat-of-combustion/lesson/Heat-of-Combustion-CHEM/