3.6 enthalpy Flashcards

1
Q

what is conservation of energy

A

energy is neither created nor destroyed but changed from one form to another

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2
Q

what are standard conditions?

A

298k
1atm

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3
Q

enthalpy of formation(^hf):

A
  • exothermic
  • enthalpy change when one one mole of a substance is formed from its elements in their standard states
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4
Q

enthalpy of combustion(^Hc):

A

enthalpy change when one mole of a substance undergoes complete combustion in oxygen.

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5
Q

Ionisation enthalpy (^Hie) first:

A
  • endothermic
  • enthalpy change when one mole of gaseous atoms loses one electron per atom to produce gaseous 1+ ions.
    e.g: Na(g) ———-> Na+(g) + e-
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6
Q

Ionisation enthalpy second:

A

when one mole of gaseous 2+ ions is produced from one mole of 1+ ions.

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7
Q

electron affinity first:

A
  • exothermic
  • produces 1 mole of gaseous ions with a -1 charge
    cl(g) + e- -> cl-(g)
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8
Q

electron affinity second:

A
  • endothermic
  • when one mole of gaseous 1- ions gains one electron to produce gaseous 2- ions.
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9
Q

enthalpy of atomisation(^Hat):
(solids and gases)

A
  • endothermic
  • when one mole of gaseous atoms is produced from an element in its normal state.
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10
Q

Hydration enthalpy:

A
  • exothermic
  • producing 1 mole of aq ions from one mole of gaseous ions
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11
Q

enthalpy of solution:

A

when an ionic solid dissolves producing an aqueous solution.

Nacl(s) + aq ——> Na+(aq) + cl- (aq)

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12
Q

Lattice enthalpy of formation:

A
  • exothermic
  • when 1 mole of an ionic compound is formed from its gaseous ions
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13
Q

Lattice breaking:

A
  • endothermic
  • breaking 1 mole of an ionic compound into its gaseous ions
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