The difference between the enthalpy of the products and the enthalpy of the reactants (KJmol-1)
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Entropy, ΔS
The dispersal of energy and disorder within the chemicals making up the chemical system (JK-1mol-1)
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Lattice enthalpy, ΔLE Hⴱ
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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First electron affinity, ΔEA1 Hⴱ
The enthalpy change that takes place when one electron is added to each atom in one mole of gaseous atoms to form one mole of gaseous 1- ions
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First ionisation energy, ΔIE1 Hⴱ
The energy required to remove one electron from each atom in one mole of gaseoues atoms of an element to form one mole of gaseous 1+ ions
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Second electron affinity, ΔEA2 Hⴱ
The enthalpy change that takes place when one electron is added to each ion in one mole of gaseous 1- ions to form one mole of gaseous 2- ions
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Second ionisation energy, ΔIE2 Hⴱ
The energy required to remove one electron from each ion in one mole of gaseous 1+ ions of an element to form one mole of gaseous 2+ ions
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Standard enthalpy change of atomisation, ΔatHⴱ
The enthalpy change that takes place when one mole of gaseous atoms forms from the element in its standard state
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Standard enthalpy change of formation, ΔfHⴱ
The enthalpy change that takes place when one mole of a compound is formed from is constituent elements in their standard states under standard conditions
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Standard enthalpy change of combustion, ΔcHⴱ
The enthalpy change that takes place when one mole of a substance reacts completely with oxygen under standard conditions with all reactants and products being in their standard states
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Standard enthalpy change of hydration, ΔhydHⴱ
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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Standard enthalpy change of neutralisation, ΔneutHⴱ
The enthalpy change that accompanies the reaction of an acid by a base to form one mole of H2O (l) under standard conditions with all reactants and products in their standard states
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Standard enthalpy change of reaction, ΔrHⴱ
The enthalpy change that accompanies a reaction in molar quantities expressed in a chemical equation under standard conditions with all reactants and products being in there standard states
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Standard enthalpy change of solution, ΔsolHⴱ
The enthalpy change that takes place when one mole of a compound is completely disssolved in water under standard conditions
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Standard solution
A solution of a known concentration
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Standard state
The physical state of a substance under standard conditions of 100kPa and a stated temperature (usually 298K)
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Standard conditions
A pressure of 100kPa, a stated temperature usually 298K (25C) and a concentration of 1moldm-3 (for reactions with aqueous solutions)
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Feasability
(Spontaneous) Describes whether the a reaction is able to happen (energetically feasible)
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Free energy change, ΔG
The balance between enthalpy, entropy and temperature for a process given by ΔG=ΔH-TΔS. A process is feasible when ΔG < 0
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Entropy change of a reaction, ΔSⴱ
ΔSⴱ = ∑Sⴱ(products) - ∑Sⴱ(reactants)
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The Gibb's equation
ΔG = ΔH - TΔS or T= ΔH / ΔS
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Entropy equation
ΔS = ΔS (surroundings) + ΔS (system)
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Other cards in this set
Card 2
Front
The dispersal of energy and disorder within the chemicals making up the chemical system (JK-1mol-1)
Back
Entropy, ΔS
Card 3
Front
The enthalpy change that accompanies the formation of one mole of an ionic compound from its gaseous ions under standard conditions
Back
Card 4
Front
The enthalpy change that takes place when one electron is added to each atom in one mole of gaseous atoms to form one mole of gaseous 1- ions
Back
Card 5
Front
The energy required to remove one electron from each atom in one mole of gaseoues atoms of an element to form one mole of gaseous 1+ ions
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