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- Enthalpy of formation (ΔHf) is the enthalpy change for the formation of 1 mol of a compound from its component elements, such as the formation of carbon dioxide from carbon and oxygen.
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What is standard enthalpy change of formation?
What is a standard enthalpy of formation H F?
How do you determine the enthalpy change for reactions?
What is enthalpy of formation?
Enthalpy of formation (\(ΔH_f\)) is the enthalpy change for the formation of 1 mol of a compound from its component elements, such as the formation of carbon dioxide from carbon and oxygen. The formation of any chemical can be as a reaction from the corresponding elements:
- 7.4: Standard Enthalpy of Formation
The standard enthalpy of formation is a measure of the...
- 8.7: Standard Enthalpy of formation
A standard enthalpy of formation \\(ΔH^\\circ_\\ce{f}\\) is...
- 7.4: Standard Enthalpy of Formation
In chemistry and thermodynamics, the standard enthalpy of formation or standard heat of formation of a compound is the change of enthalpy during the formation of 1 mole of the substance from its constituent elements in their reference state, with all substances in their standard states.
The definition of standard enthalpy of formation is the change in enthalpy when one mole of a substance is formed in its standard state from its constituent elements in their standard state at 298k and 1 atm. Since elements like Oxygen are in their standard state, there is no standard enthalpy of formation to talk about here. ( 25 votes) Upvote.
- 16 min
- Sal Khan
Calculate enthalpy changes for various chemical reactions. Explain Hess’s law and use it to compute reaction enthalpies. Thermochemistry is a branch of chemical thermodynamics, the science that deals with the relationships between heat, work, and other forms of energy in the context of chemical and physical processes.
The standard enthalpy of formation, also known as the heat of formation, is the enthalpy change when 1 mole of a pure substance forms from its constituent elements at standard temperature and pressure.
