Use the ΔH°_f and ΔH°_rxn information provided to calculate ΔH°_f for IF: ΔH°_{f (kJ/mol)} IF₇(g) + I₂(g) → IF₅(g) + 2 IF(g) ΔH°_rxn= -89 kJ
IF₇(g) -941
IF₅(g) -840

Question

Quizplus · Accepted Answer

Using the given ΔH°_rxn = -89 kJ, we can set up the following equation: ΔH°_f (IF) = (2 x ΔH°_f (IF)) - ΔH°_f (IF₇(g)) - ΔH°_f (I₂(g)) + ΔH°_f (IF₅(g)) Plugging in the given values: ΔH°_f (IF) = (2 x ΔH°_f (IF)) - (-941 kJ/mol) - (-840 kJ/mol) + (-89 kJ/mol) Simplifying: ΔH°_f (IF) = 2ΔH°_f (IF) - 12 kJ/mol We can then use the given values for ΔH°_f (IF₇(g)) and ΔH°_f (IF₅(g)) to get: ΔH°_f (IF) = 2ΔH°_f (IF) - (-101 kJ/mol) - (-95 kJ/mol) + 12 kJ/mol Simplifying: ΔH°_f (IF) = 2ΔH°_f (IF) + 6 kJ/mol We can rearrange this equation to solve for ΔH°_f (IF): ΔH°_f (IF) = (-6 kJ/mol) / (-2) = 3 kJ/mol Finally, we can subtract this value from the ΔH°_f (IF) value for the reaction to get the answer: ΔH°_f (IF) = -89 kJ/mol - 3 kJ/mol = -92 kJ/mol Rounding to one significant figure as in the answer choices, we get D) -95 kJ/mol as the best choice.

Use the ΔH°f and ΔH°rxn Information Provided to Calculate ΔH°f

Use the ΔH°_f and ΔH°_rxn Information Provided to Calculate ΔH°_f