a. Use the H f and H rxn information provided to calculate H f for IF: IF

a. Use the ΔH°_f and ΔH°_rxn information provided to calculate ΔH°_f for IF:

IF₇ (g) + I₂ (g) → IF₅ (g) + 2 IF (g) ΔH°_rxn = –89 kJ/mol

	IF7 (g)	IF5 (g)
ΔH°f (kJ/mol)	–937	–851

b. Consider the production of HCl from chlorine and hydrogen:

Cl₂ (g) + H₂ (g) → 2 HCl (g)

Calculate ΔH for the reaction, using the data from the table of average bond dissociation energies.

Answer rating: 100% (QA)

To solve both parts well use Hesss Law which states that the overall enthalpy change of a reaction i... View the full answer