Calculating ΔH°rxn problem! - Chemistry?
Oxidation of gaseous ClF by F2 yields liquid ClF3, an important fluorinating agent. Use the following thermochemical equations to calculate ΔH°rxn for the production of ClF3.
(1) 2 ClF(g) + O2(g) → Cl2O(g) + OF2(g) ΔH° = 167.5 kJ
(2) 2 F2(g) + O2(g) → 2 OF2(g) ΔH° = -43.5 kJ
(3) 2 ClF3(l) + 2 O2(g) → Cl2O(g) + 3 OF2(g) ΔH° = 394.1 kJ
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leave 1 and 2 untouched. flip 3 to put ClF3 on product side.
the result:
(1) 2 ClF(g) + O2(g) → Cl2O(g) + OF2(g) ΔH° = 167.5 kJ
(2) 2 F2(g) + O2(g) → 2 OF2(g) ΔH° = -43.5 kJ
(3) Cl2O(g) + 3 OF2(g) → 2 ClF3(l) + 2 O2(g) ΔH° = -394.1 kJ
Add everything up and cancel out like items:
2 ClF(g) + 2 F2(g) → 2 ClF3(l) ΔH° = -270.1 kJ
Divide through by 2:
ClF(g) + F2(g) → ClF3(l) ΔH° = -135 kJ
using 135 kJ for the answer seems best.