2. Great thanks to
JONATHAN HOPTON & KNOCKHARDY PUBLISHING
www.knockhardy.org.uk/sci.htm
Some taken from
ENTHALPY
CHANGES
3. “The overall enthalpy change of a chemical process is
independent of the path taken”
The enthalpy change going from A to B can be found by
adding the values of the enthalpy changes for the reactions
A to X, X to Y and Y to B.
ΔHr = ΔH1 + ΔH2 + ΔH3
HESS’S LAW
4. Dissolving solid sodium
hydroxide in water
This process produces sodium and
hydroxide ions ie. NaOH (aq)
solution.
1. NaOH(s) + H2O NaOH (aq) + H2O ΔH1
Consider three reactions
5. Reacting the sodium hydroxide
solution with a hydrochloric acid
solution = neutralization
Na+ OH-
2. NaOH (aq) +HCl (aq) NaCl (aq) + H2O ΔH2
7. Recap:
1. NaOH(s) + H2O NaOH (aq) + H2O ΔH1
2. NaOH (aq) +HCl (aq) NaCl (aq) + H2O ΔH2
3. NaOH(s) + HCl (aq) NaCl (aq) + H2O ΔH3
Show that equation 1 plus equation 2 is the same as equation 3
What conclusion about enthalpy can be made?
8. Equation 1 + 2
1. NaOH(s) + H2O NaOH (aq) + H2O ΔH1
2. NaOH (aq) +HCl (aq) NaCl (aq) + H2O ΔH2
3. NaOH(s) + HCl (aq) NaCl (aq) + H2O ΔH3
Combined – equations 1 and 2 give equation 3
Since the equation 1 then 2 sequence starts and
finishes with the same reactants and products as
equation 3, Hess’s Law says ΔH3 = ΔH1 + ΔH2