Enthalpy definitions OCR F325

Flashcards with definitions for enthalpy, taken from the OCR A2 textbook

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Lattice enthalpy

Lattice enthalpy is the enthalpy change that accompanies the formation of one mole of an ionic compound from its gaseous ions under standard conditions.

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Hess' Law

Hess' law states that if a reaction can take place by more than one route and the initial and final conditions are the same, the total enthapy change is the same for each route.

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Standard enthalpy change of formation

The standard enthalpy change of formation is the enthalpy change that takes place when one mole of a compound is formed from its constituent elements in their standard states under standard conditions.

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Enthalpy change of atomisation

The enthalpy change of atomisation is the enthalpy change that takes place when one mole of gaseous atoms forms from the element in its standard state.

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First ionisation energy/second ionisation energy

First ionisation energy is the amount of energy required to remove one electron from each atom in one mole of gaseous atoms/one mole of gaseous +1 ions, forming one mole of gaseous +1 ions/one mole gaseous +2 ions.

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First electron affinity/second electron affinity

The first electron affinity is the enthalpy change accompanying the addition of one electron to each atom in one mole of gaseous atoms/ to each ion in one mole gaseous 1- ions to form one mole of gaseous 1- ions/ to form one mole of gaseous 2- ions.

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Standard enthalpy change of solution

The standard enthalpy change of solution is the enthalpy change that takes place when one mole of a compound is completely dissolved in water under standard conditions.

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Standard enthalpy change of hydration

The standard enthalpy change of hydration is the enthalpy change that takes place when one mole of isolated gaseous ions is dissolved in water forming one mole of aqueous ions under standard conditions.

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