Enthalpy Change - Definitions (Edexcel International AS Chemistry): Revision Note
Exam code: XCH11
Enthalpy Change - Definitions
To be able to compare the changes in enthalpy between reactions, all thermodynamic measurements are carried out under standard conditions
These standard conditions are:
A pressure of 100 kPa (you may see some older exam questions that use a figure of 101 kPa; 101 325 Pa is one atmosphere, but the standard pressure is now defined as exactly 100 kPa)
A temperature of 298 K (25 oC)
Each substance involved in the reaction is in its standard physical state (solid, liquid or gas)
To show that a reaction has been carried out under standard conditions, the symbol ‘Ꝋ’ is used
ΔHꝊ = the standard enthalpy change
There are a number of standard definitions relating to enthalpy changes that you are expected to know
Enthalpy Definitions Table
Standard enthalpy change of reaction, ΔHrꝊ (exothermic or endothermic): the enthalpy change when the reactants in the stoichiometric equation react to give the products under standard conditions
Standard enthalpy change of formation, ΔHfꝊ (exothermic or endothermic): the enthalpy change when one mole of a compound is formed from its elements under standard conditions
Standard enthalpy change of combustion, ΔHcꝊ (exothermic): the enthalpy change when one mole of a substance is burnt in excess oxygen under standard conditions
Standard enthalpy change of neutralisation, ΔHneutꝊ (exothermic): the enthalpy change when one mole of water is formed by reacting an acid and an alkali under standard conditions
A further definition that is expected knowledge, although less used at AS level, is:
Standard enthalpy of atomisation - the enthalpy change when one mole of gaseous atoms is formed from an element in its standard state, under standard conditions
Examiner Tips and Tricks
You will see various enthalpy change symbols used with subtle changes, e.g.
ΔHcꝊ or ΔcHꝊ for enthalpy of combustion
Whichever symbol you use must have the following basic points:
Δ to represent change
H to represent enthalpy
Ꝋ to represent standard conditions
A symbol to represent the type of enthalpy change occurring, e.g.
c for combustion
f for formation
neut for neutralisation
r for reaction
Worked Example
Calculating the enthalpy change of reaction
One mole water is formed from hydrogen and oxygen, releasing 286 kJ of energy
H2 (g) + ½O2 (g) → H2O (l) ΔHrꝊ = -286 kJ mol-1
Calculate ΔHrꝊ for the reaction below:
2H2 (g) + O2 (g) → 2H2O (l)
Answer
Since two moles of water molecules are formed in the question above, the energy released is simply:
ΔHrꝊ = 2 mol x (-286 kJ mol-1) = -572 kJ mol-1
Worked Example
Calculating the enthalpy change
Calculate ΔHrꝊ for the reaction below, given that ΔHfꝊ [Fe2O3(s)] = -824.2 kJ mol-1
4Fe(s) + 3 O2(g) → 2 Fe2O3(s)
Answer
Since two moles of Fe2O3 (s) are formed the total change in enthalpy for the reaction above is:
ΔHrꝊ = 2 x (-824.2 kJ mol-1) = -1648 kJ mol-1
Worked Example
Calculating enthalpy changes
Identify each of the following as ΔHrꝊ, ΔHfꝊ, ΔHcꝊ or ΔHneutꝊ
MgCO3 (s) → MgO (s) + CO2 (g)
C (graphite) + O2 (g) → CO2 (g)
HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l)
Answer
Answer 1: ΔHrꝊ
Answer 2: ΔHfꝊ as one mole of CO2 is formed from its elements in standard state and ΔHcꝊ as one mole of carbon is burnt in oxygen
Answer 3: ΔHneutꝊ as one mole of water is formed from the reaction between an acid and an alkali
Examiner Tips and Tricks
The ΔHfꝊ of an element in its standard state is zero.
For example, ΔHf Ꝋ of O2(g) is 0 kJ mol-1
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