Introducing Entropy (Edexcel A Level Chemistry): Revision Note

Introducing Entropy

• You may have wondered why it is that endothermic reactions occur at all, after all, what can be the driving force behind endothermic reactions if the products end up in a less stable, higher energy state?

• Although the majority of chemical reactions we experience everyday are exothermic,  ΔH^ꝋ alone is not enough to explain why endothermic reactions occur

The driving force behind chemical reactions cannot be explained by enthalpy changes alone as it makes not sense for chemical to end up in a less stable higher energy state in endothermic reactions

• The answer is entropy

Chaos in the universe

• The entropy (S) of a given system is the number of possible arrangements of the particles and their energy in a given system

  • In other words, it is a measure of how disordered or chaotic a system is

• When a system becomes more disordered, its entropy will increase

• An increase in entropy means that the system becomes energetically more stable

• An example of a system that becomes more disordered is when a solid is melted

• For example, melting ice to form liquid water:

H₂O (s) → H₂O (l)

• The water molecules in ice are in fixed positions and can only vibrate about those positions

• In the liquid state, the particles are still quite close together but are arranged more randomly, in that they can move around each other

• Water molecules in the liquid state are therefore more disordered

• Thus, for a given substance, the entropy increases when its solid form melts into a liquid

• In both examples, the system with the higher entropy will be energetically favourable (as the energy of the system is more spread out when it is in a disordered state)

Melting a solid will cause the particles to become more disordered resulting in a higher entropy state

Entropy Changes

Production of a gas

• During the thermal decomposition of calcium carbonate (CaCO₃) the entropy of the system increases:

CaCO₃ (s) → CaO (s) + CO₂ (g)

• In this decomposition reaction, a gas molecule (CO₂) is formed

• The CO₂ gas molecule is more disordered than the solid reactant (CaCO₃), as it is constantly moving around

• As a result, the system has become more disordered and there is an increase in entropy

• Another example is the reaction of ethanoic acid with ammonium carbonate

(NH₄)₂CO₃ (s) + 2CH₃COOH (aq) → 2CH₃COO^- (aq) + 2NH₄⁺ (aq) + CO₂ (g) + H₂O (l) 

• There is a slight fall in temperature during the reaction indicating the process is endothermic

  • Energy is taken in from the surroundings

• The particles are well-ordered in the solid, and the disorder increases because a solution and, especially, a gas is formed so entropy increases during the reaction

Dissolving a solid

• When ammonium nitrate is dissolved in water, the temperature of the solution decreases, therefore the process is endothermic

  • Energy is taken in from the surroundings

NH₄NO₃ (s) + aq → NH₄⁺ (aq) + NO₃^- (aq)    ΔH = 25.7 kJ mol^-1

• The level of disorder increases as the particles are no longer in a fixed position and are now free to move

• However, it is not always this simple!

• When an ionic solid dissolves

  • Bonds between the particles are broken increasing the disorder and taking in energy 

  • Bonds between the solvent and particles are made reducing the disorder and releasing energy

• Therefore it is difficult to predict whether the process will be endothermic or exothermic 

Endothermic reactions between two solids 

• When barium hydroxide and ammonium chloride are mixed, they form a paste and the temperature drops significantly 

• Therefore this is an endothermic process

  • Energy is taken in from the surroundings

2NH₄Cl (s) + Ba(OH)₂.8H₂O (s)  → BaCl₂.2H₂O (s) + 2NH₃ (g) + 8H₂O (l)

• The gas produced is ammonia and this can be detected by the smell and it will turn damp red litmus paper blue

• When two solids are mixed and react together, the entropy change will depend on the physical state of the compounds made and not just on the energy changes in the reaction

• Two solids will of course have a very low entropy due to the high order 

• If a liquid or gas is produced the entropy will have increased due to the increased disorder of the particles