thermodynamics Flashcards

1
Q

What does Hess’s Law state?

A
  • the enthalpy change for a reaction is independent of the route taken .
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2
Q

Define standard enthalpy of formation. (ΔHf)

A
  • the enthalpy change when one mole of a compound is formed from its constituent elements in standard conditions, with all products + reactants in standard states.
  • e.g = Na (s) + 1/2Cl2 (g) —> NaCl (s)
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3
Q

Define standard enthalpy of combustion. (ΔH°c)

A
  • the enthalpy change when one mole of a substance is completely burnt in (excess) oxygen.
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4
Q

Define enthalpy of atomisation. (ΔHat)

A
  • the enthalpy change when one mole of gaseous atoms is formed from a compound in its standard state in standard conditions (endothermic .)

e.g = Na (s) —> Na (g)

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5
Q

Define first ionisation energy. (ΔHi)

A

the enthalpy change when one mole of electrons is removed from one mole of singly charged ions —> produce doubly charged ions - second ionisation energy.

1st = M(g) —> M(g) + e-
2nd = M
(g) —> M^2+ (g) + e-

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6
Q

Define the first electron affinity. (EA1)

A
  • enthalpy change when one mole of gaseous atoms gain one mole of electrons to form one mole of gaseous 1- ions.

e.g - Cl (g) + e- —> Cl- (g)

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7
Q

Define second electron affinity. (EA2)

A
  • enthalpy change when one mole of gaseous 1- ions gain one mole of electrons to form one mole of gaseous 2- ions.
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8
Q

Define lattice enthalpy of formation. (ΔH ⦵ LE)

A
  • enthalpy change when one mole of solid ionic compound/ crystalline compound formed from its constituents gaseous ions
  • scattered infinite distance apart
    M^+ (g) + X^- (g) —> MX (s)
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9
Q

Define lattice enthalpy of dissociation. (ΔH°)

A
  • enthalpy change when one mole of solid ionic lattice is broken up to produce gaseous ions in an infinite distance apart .
  • e.g = MX (s) —> M^+ (g) + X^- (g)
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10
Q

what does the value of a lattice enthalpy depend on?

A
  • the charges on the ions
  • the size of the ions
  • the type of lattice formed (pattern which they pack together)
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11
Q

Define mean bond dissociation enthalpy

A

enthalpy change when one mole of (a certain type of) covalent bonds is broken, with all species in the gaseous state.

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12
Q

Define mean bond dissociation enthalpy

A

enthalpy change when one mole of (a certain type of) covalent bonds is broken, with all species in the gaseous state.

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