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Enthalpy Change (ΔH)
The amount of energy released or absorbed during a chemical reaction.
Exothermic Reaction
A reaction that releases energy into the surroundings, indicated by a negative ΔH.
Endothermic Reaction
A reaction that absorbs energy from the surroundings, indicated by a positive ΔH.
Activation Energy (Ea)
The minimum energy required for a reaction to take place.
Standard Conditions
Conditions defined as 100 kPa, 298 K (25°C), and 1 mol dm-3 for solutions, under which ΔH values are measured.
Standard Enthalpy Change of Reaction (ΔrH)
The enthalpy change associated with a stated reaction in mole quantities shown in the chemical equation under standard conditions.
Standard Enthalpy Change of Formation (ΔfH)
The enthalpy change associated with the formation of 1 mole of a compound from its elements under standard conditions.
Standard Enthalpy Change of Combustion (ΔcH)
The enthalpy change for the complete combustion of 1 mole of a substance under standard conditions.
Standard Enthalpy Change of Neutralisation (ΔneutH)
The enthalpy change associated with the formation of 1 mole of water from a neutralisation reaction between an acid and a base.
Conservation of Energy
Energy cannot be created or destroyed; it can only be transferred between the system and the surroundings.
Note 
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