CIE AS Chemistry (9701) exams from 2022

Revision Notes

1.5.1 Enthalpy Change, ΔH

Enthalpy Changes

  • The total chemical energy inside a substance is called the enthalpy (or heat content)
  • When chemical reactions take place, changes in chemical energy take place and therefore the enthalpy changes
  • An enthalpy change is represented by the symbol ΔH (Δ= change; H = enthalpy)
  • An enthalpy change can be positive or negative

Exothermic reactions

  • A reaction is exothermic when the products have less enthalpy than the reactants
  • Heat energy is given off by the reaction to the surroundings
    • The temperature of the environment increases
    • The temperature of the system decreases
  • There is an enthalpy decrease during the reaction so ΔH is negative
  • Exothermic reactions are thermodynamically possible (because the enthalpy of the reactants is higher than that of the products)
  • However, if the rate is too slow, the reaction may not occur. In this case the reaction is kinetically controlled

Chemical Energetics Exothermic Reaction, downloadable AS & A Level Chemistry revision notes

The enthalpy change during an exothermic reaction

Endothermic reactions

  • A reaction is endothermic when the products have more enthalpy than the reactants
  • Heat energy is absorbed by the reaction from the surroundings
    • The temperature of the environment decreases
    • The temperature of the system increases
  • There is an enthalpy increase during the reaction so ΔH is positive

Chemical Energetics Endothermic Reaction, downloadable AS & A Level Chemistry revision notes

The enthalpy change during an endothermic reaction

Exam Tip

It is important to specify the physical states of each species in an equation when dealing with enthalpy changes as any changes in state can cause very large changes of enthalpy.

For example:

Na+Cl (s) → Na+ (aq) + Cl (aq)   ΔH = +4 kJ mol-1

Na+Cl (g) → Na+ (g) + Cl (g)   ΔH = + 500 kJ mol-1

Also, remember that the system is the molecules that are reacting (ie. the reaction itself) and the surroundings is everything else (eg. the flask the reaction is taking place in).

Author: Francesca

Fran has taught A level Chemistry in the UK for over 10 years. As head of science, she used her passion for education to drive improvement for staff and students, supporting them to achieve their full potential. Fran has also co-written science textbooks and worked as an examiner for UK exam boards.
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