🤓 Based on our data, we think this question is relevant for Professor Amateis' class at VT.
Reaction of gaseous ClF with F 2 yields liquid ClF3, an important fluorinating agent. Use the following thermochemical equations to calculate ΔH°rxn for this reaction:
(1) 2CIF(g) + O2(g) ⟶ Cl2O(g) + OF2(g) ΔH°rxn = 167.5 kJ
(2) 2F2(g) + O2(g) ⟶ 2OF2(g) ΔH°rxn = −43.5 kJ
(3) 2ClF3(l) + 2O2(g) ⟶ Cl2O(g) + 3OF2(g) ΔH°rxn = 394.1 kJ
2ClF + 2F2 ⟶ 2ClF3
To find the ΔHrxn, we need to use the Hess's Law where we have to rearrange the given equations to get the desired reaction.