The heat content that is stored in a chemical system. Enthalpy can't be measured but enthalpy changes can.
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Enthalpy change
delta H=products-reactants
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Exothermic
Energy loss by the chemical system to the surroundings. delta H is negative.
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Endothermic
Energy gain by the chemical system from the surroundings. delta H is positive.
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Activation energy
The minimum energy required for a reaction to take place
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Standard state
The physical state of a substance under standard conditions
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Standard enthalpy change of reaction
The enthalpy change that accompanies a reaction in the molar quantities shown in a chemical equation under standard conditions and standard states
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Standard enthalpy change of formation
The enthalpy change that takes place when one mole of product is formed from its elements under standard conditions and in standard states
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Standard enthalpy change of combustion
The enthalpy change that takes place when one mole of a substance reacts completely with oxygen under standard conditions and in standard states.
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Standard enthalpy change of neutralisation
The energy change that accompanies the reaction of an acid and a base to form one mole of water under standard conditions and in standard states. The value for the enthalpy change of neutralisation is the same for all neutralisation reactions.
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Specific heat capacity
The energy required to raise the temperature of 1g of a substance by 1K
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Average bond enthalpy
The energy required to break one mole of a specified type of bond in a gaseous molecule
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Other cards in this set
Card 2
Front
delta H=products-reactants
Back
Enthalpy change
Card 3
Front
Energy loss by the chemical system to the surroundings. delta H is negative.
Back
Card 4
Front
Energy gain by the chemical system from the surroundings. delta H is positive.
Back
Card 5
Front
The minimum energy required for a reaction to take place
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