The variations together with the heat content of the materials which react, result in enthalpy(H) the accurate word for heat content. Typically, this variation in the heat content or enthalpy is displayed by an alteration in temperature. There is an alteration in the heat of the reaction, during the reaction. The enthalpy change for the reaction is represented by ΔH (sometimes called the heat of reaction). The enthalpy of products is H2 and is less than the heat content of reactants H1.
Enthalpy Formula is denoted as
Enthalpy Change = Heat of the Reaction
As the enthalpy change amplifies itself as heat, the statement “heat of reaction” is frequently made use of in place of enthalpy change of the reaction. The key relation between enthalpy change and heat of reaction. The enthalpy of reaction equals the heat of reaction at constant pressure.
Problem 1: For the thermite reaction compute the enthalpies of formation.
2Al + Fe2O3 àAl2O3 + 2Fe
This reaction occurs when a mixture of powders aluminium and iron(III) oxide is ignited with a magnesium fuse.
ΔH for Fe2O3 = -826kJ/mol
ΔH for Al2O3 = -1676 kJ/mol
ΔH for Al = ΔH for Fe = 0
We use the equation.
ΔH (reaction) = ΔH for Al2O3 – ΔH for Fe2O3
ΔH (reaction) = -1676kJ – (-826kJ)
ΔH (reaction) = -850kj
Problem 2: For a combustion reaction.
2C8H18 + 25CO2 à 16CO2 + 18H2O
What is the variation in enthalpy of the reaction?
ΔH for CO2 = -394kJ
ΔH for H2O = -286kJ
ΔH for C8H18 = -269kJ
ΔH = 16 times ΔH for CO2 + 18 times ΔH for H2O – 2 times ΔH for C8H18
ΔH = 16 times (-394kJ) + 18 times (-286kJ) – 2 times (-269kJ)
ΔH = -1.09 times 104kJ