2 H2(g) + O2(g) → 2 H2O(l)
Note that we need to multiply each ΔH˚f by the stoichiometric coefficient since ΔH˚f is in kJ/mol.
Also, note that ΔH˚f for elements in their standard state is 0.
ΔH˚f H2(g) = 0 kJ/mol
Consider the reaction: 2 H2(g) + O2(g) → 2 H2O(l). Use the enthalpies of formation in Appendix C to determine the true reaction enthalpy.
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