Thermodynamics Flashcards

1
Q

Define enthalpy of formation

A

enthalpy change when 1 mol of a compound is formed from its elements in standard states under standard conditions

EXO

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2
Q

Define enthalpy of atomisation

A

enthalpy change when 1 mol of gaseous atoms are formed from an element in its standard states

ENDO

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3
Q

Define enthalpy of 1st ionisation energy

A

enthalpy change when 1 mol of gaseous ions is formed from 1 mol of gaseous atoms

ENDO

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4
Q

Define enthalpy of 2nd ionisation energy

A

enthalpy change when 1mol of gaseous 2+ ions are formed from 1mol of gaseous 1+ atoms

ENDO

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5
Q

Enthalpy of 1st electron affinity

A

enthalpy change when 1 mol of gaseous 1- ions formed from 1 mol of gaseous atoms

EXO

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6
Q

Enthalpy of 2nd electron affinity

A

enthalpy changed when 1 mol gaseous 2- ions are formed from 1 mol of gaseous 1- ions

ENDO

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7
Q

Enthalpy of lattice formation

A

enthalpy change when 1 mol of solid ionic compound is formed from its gaseous ions

EXO

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8
Q

enthalpy of hydration

A

enthalpy change when 1 mol of aqueous ions are formed from 1 mol of gaseous ions.

EXO

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9
Q

Enthalpy of solution

A

enthalpy change when 1 mol of solute is dissolved in enough solvent that no further enthalpy change occurs in further dilution

ENDO,EXO

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10
Q

enthalpy of lattice dissociation

A

enthalpy change when 1 mol of ionic compound separates into its gaseous ions

ENDO

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11
Q

when do you add a 2nd electron affinity(ea) or 2nd ionisation enthalpy(ie) to your born-haber cycle

A

if there is a 2- ion a 2nd ea is needed

if there is a 2+ ion a 2nd ie

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12
Q

When will a reaction be feasible in ∆G

A

if ∆G is negative -reaction feasible

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13
Q

Give ∆G equation

A

∆G = ∆H - T∆S

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14
Q

How can you change numbers in equation to make reaction feasible

A

Increase entropy-> more positive ∆S

Reaction exo –>more negative ∆H

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15
Q

Why is enthalpy change of A larger than enthalpy change of B.

A

has larger radius/more shells
increased shielding
less powerful attraction (of nucleus) for (outer) e- in B

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16
Q

What 2 factors affect enthalpy of lattice formation

A

Ion Size
The larger the ions, the less negative the enthalpies of lattice formation
(i.e. a weaker lattice). As the ions are larger charges further
apart so have a weaker attractive force between them.

Charge of Ion
bigger the charge of the ion, the greater the attraction between the
ions so the stronger the lattice enthalpy (more negative values).