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Simple Explanation:
Introduction to Bond Enthalpy
Bond Enthalpy: The energy (kJ/mol) required to break a covalent bond between two atoms.
A higher bond enthalpy means a more stable bond.
Average Bond Enthalpy Chart
This chart shows the rough estimates based on the energy required to break a specific but similar bond in various compounds.
Standard Enthalpies of Formation Chart
This chart shows how much energy is needed to form the bonds of a compound from its constituent elements in their standard state.
TO BE ADDED
Bond Enthalpy Calculations
Bond Enthalpy Formula:
This formula is used for calculating the energy (KJ/mol) released during a chemical reaction in regards to the covalent bonds broken and formed. Use the average bond enthalpy chart as a reference.
ΔH° = ΣH°(Bonds Broken) - ΣH°(Bonds Formed)
ΔH: Enthalpy change (kJ/mol)
ΣH: Sum of bond enthalpy broken/formed.
Note: The degrees symbol (°) indicates that the values are based on standard ambient temperature (25°C/298 K) and pressure (1 atm).
Heat of Formation Formula:
This formula is used for calculating the energy (KJ/mol) released during a chemical reaction in regards to the enthalpy changes of reactants and products. Use the standard enthalpies of formation chart as a reference.
ΔH°rxn = ΣΔH°f (Products) - ΣΔH°f (Reactants)
ΔH: Enthalpy change (kJ/mol)
ΣΔHf: Sum of the standard enthalpies of formation for products/reactants.
Negative values for ΔH mean that the process is exothermic, which is often favorable.
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