Revision:Energetics - 16

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16.1 Standard enthalpy changes of reaction

16.1.1

Standard state -- 101 kPa, 298 K (or 1 atm, 25 degrees Celsius).

Standard enthalpy change of formation -- The enthalpy change when 1 mol of a substance is made from its elements in their standard states eg

.

(molecules, like H₂ are considered to be 'standard state'. Fractions of mols -> ie fractions in coefficients, may also be used if necessary as 1 mol must be produced).

16.1.2

If a reaction can be expressed in terms of changes of formation (and bond enthalpies as in SL) then add up all the values to get the for the reaction.

16.2 Lattice enthalpy

16.2.1

Lattice enthalpy - the enthalpy change when 1 mol of crystals (ie an ionic lattice) is formed from its component particles at an infinite distance apart. ie:

.

The value of lattice enthalpy is assumed to be positive for the separation of the lattice, and negative for the formation of the lattice.

This is because energy is released when ionic bonds are formed (exothermic) and energy is absorbed to break the bonds (endothermic).

16.2.2

As above, lattice enthalpies just add another type of reaction to those which can be shown on the Born-Harber cycle.

16.2.3

lattice enthalpy increases with higher ionic charge and with smaller ionic radius (due to increased attraction).

16.3 Entropy

16.3.1

Factors which increase disorder in a system : Mixing of particles, change of state to greater distance between particles (solid --> liquid or liquid --> gas), increased particle movement (temperature), increased number of particles (when more gas particles are produced, this generally outweighs all other factors).

16.3.2

Predict the sign of (the change in entropy) for a reaction based on the above factors. is positive when entropy increases (more disorder) and negative when entropy decreases (less disorder).

16.3.3

The standard entropy change can be calculated by subtracting the absolute entropy of the reactants from that of the products.

16.4 Spontaneity of a reaction

16.4.1

Reactions which release heat (and so increase stability) tend to occur. Reactions which increase entropy ( is positive) tend to occur, but neither can be used to accurately predict spontaneity alone.

16.4.2

when is negative, the reaction is spontaneous, when it's positive, their reaction is not.

16.4.3

• denotes change in Gibb's free energy.

spontaneity depends on , and the temp (, in Kelvin) at which the reaction takes place (or doesn't as the case may be).

16.4.4

Yeah...well...stick numbers into that equation above...

16.4.5

4 possibilities...

1. is always negative when is negative and is positive.
2. is negative at high temperatures if is positive and is positive (ie an endothermic reaction is spontaneous when is greater than )
3. is negative at lower temperatures if is negative and is negative (exothermic reactions are spontaneous if is bigger than )
4. is never negative if is positive and negative.

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