Reactions that involve losing/releasing heat energy to the surrounding.
ΔH= (-ve)
Surrounding temperature increases
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Endothermic Reactions
A reaction that absorbs heat energy from the surrounding.
ΔH= (+ve)
Surrounding temperature decreases.
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Standard enthalpy change of Reaction
The enthalpy change in molar quantities that are expressed in a chemical equation under standard conditions.
Pressure- 100kPa
Temperature- 298K (25c)
Concentrations( Only aqueous)- 1 mol/dm3
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Standard enthalpy change of Combustion
The enthalpy change when 1 mole of a substance is burned completely with oxygen under standard conditions.
Pressure- 100kPa
Temperature- 298K (25c)
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Standard enthalpy change of Neutralisation
The enthalpy change when one mole of water is produced by the neutralisation of an acid with an alkali under standard conditions.
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Standard enthalpy change of Formation
The enthalpy change when one mole of a compound is formed from its elements in their standard state, under standard conditions.
The standard enthalpy change of formation of an element is always 0.
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Standard enthalpy change of Atomization
ΔatH
It is the enthalpy change when one mole of a gaseuous atom is formed from its element in its standard state, under standard conditions.
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Bond enthalpy
The enthalpy change when 1 mole of a bond in the gaseous state is broken.
Average bond enthalpy is the enthalpy change when 1 mole of a bond averaged out over many different molecules is broken.
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Hess' Law
Hess' law states that the enthalpy change of a reaction is independent of the path taken in converting reactants into products, provided the intial and the final conditions are the same in each case.
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