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level: Year 2 enthalpy, entropy and free energy

Questions and Answers List

level questions: Year 2 enthalpy, entropy and free energy

QuestionAnswer
What is lattice enthalpythe formation of one mole of an ionic compound from its gaseous ion under standard conditions
The standard enthalpy of atomisationformation of one mole of gaseous atoms from the element in its standard states under standard conditions.
standard enthalpy of formationwhen one mole of a compound is formed from its consituent elements in standard states under standard conditions
first ionisation energyremoval of one electron from one mole of gaseous atoms to form one mole of gaseous plus ions
enthalpy change of solutionone mole of a compound is dissolved in water under standard conditions
q=mc delta T
BREAKING UP a lattice =endothermic
formation of lattice =exothermic
the standard enthalpy change of hydrationone mole of gaseous ions is dissolved in water forming mole of aqueous ions under standard c
factors affecting hydrationionic size -ionic radius increases attraction between ions and water decreases hydration enegry is more possitive ionic charge - ionic charge increases attraction with water mols increase so hydration energy is more negative
how to recognise lattice enthalpy by state symbolsgaseous to solid
The first electron affinitythe addition of one electron to each atom in one mol of gaseous atoms to form 1-
What are key features of lattice enthalpy-exothermic change indicates strength of ionic lattice bond strength
formation of lattice is exo or endoexo
breaking of latticeendothermic
second ionisation energythe removal one of one elctron form each ion in mole of gaseous 1+ ions to form mole of gaseous 2+ ions
Working out enthalpy change of solutioncalculate energy change in solution by q=mcdeltaT calculate the moles work out delta of solution by q/ moles