Enthalpy Change & Cycles Flashcards

(10 cards)

1
Q

Define enthalpy change of lattice formation (∆HLF)

A

Heat energy change when 1 mol solid ionic compound formed from it’s (g) ions

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2
Q

Outline the meaning of exothermic and endothermic reactions

A

Exothermic = heat energy released/bonds made
Endothermic = heat energy taken in/bonds broken

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3
Q

Define ∆H formation (∆HF)

A

Heat energy change of compound formed from it’s elements

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4
Q

Define ∆H of atomisation (∆Hat)

A

Heat energy change when 1 mol (g) atoms formed from it’s elements in the standard state

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5
Q

Define the ∆H of 1st ionisation energy (∆HIE)

A

Heat energy change when 1 mol of e- lost from 1 mol of (g) atoms

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6
Q

Define the ∆H of 2nd ionisation energy (∆HIE2)

A

Heat energy change when 1 mol of e- taken from 1 mol of (g)

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7
Q

Define the ∆H of 1st e- affinity (∆HEA)

A

Heat energy change when 1 mol of e- is added to 1 mol (g) atoms

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8
Q

Define the ∆H of the 2nd e- affinity (∆HEA2)

A

Heat energy change when 1 mol of e- added to 1 mol (g) ions

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9
Q

Outline the standard enthalpy change of formation equation (ΔH°f)

A
  1. Write out equation at top with constituent elements below
  2. Input the arrows into diagram (ensure the head is the right way round)
  3. Input values and calculate ΔH°f
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10
Q

Outline the difference between the arrow directions for the equations of (ΔH°f) and (ΔH°c)

A

(ΔH°f) = bottom to top
(ΔH°c) = top to bottom

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