Enthalpy changes for the following reactions can be determined experimentally:
C2H4(g) + 3 O2(g) → 2 CO2(g) + 2 H2O(l)
C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(l)
ΔHorxn = -1411.1 kJ/mol-rxn
ΔHorxn = -1367.5 kJ/mol-rxn
Use the given values to determine the enthalpy change for the
reaction:
C2H4(g) + H2O(l)
→ C2H5OH(l)
ΔHorxn (answer) = kJ/mol-rxn
Lets number the reaction as 1, 2, 3 from top to bottom
required reaction should be written in terms of other reaction
This is Hess Law
required reaction can be written as:
reaction 3 = +1 * (reaction 1) -1 * (reaction 2)
So, ΔHo rxn for required reaction will be:
ΔHo rxn = +1 * ΔHo rxn(reaction 1) -1 * ΔHo rxn(reaction 2)
= +1 * (-1411.1) -1 * (-1367.5)
= -43.6 KJ
Answer: -43.6 KJ
Enthalpy changes for the following reactions can be determined experimentally: C2H4(g) + 3 O2(g) → 2...
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