Problem: Gaseous hydrogen and fluorine combine in the reaction below to form hydrogen fluoride:H2(g) + F2(g) → 2 HF(g)        ΔH°rxn = -540 kJWhat is the value of the heat of formation for HF(g)?A) -1080 kJ/molB) -540 kJ/molC) -270 kJ/molD) 270 kJ/molE) 540 kJ/mol

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We’re being asked to determine the standard enthalpy change of formation (ΔH˚f) for HF(g)


Recall that ΔH˚rxn can be calculated from the enthalpy of formation (ΔH˚f) of the reactants and products involved


ΔH˚rxn = ΔH˚f, products - ΔH˚f, reactants


We’re given the ΔH˚rxn for the combustion of 1 mole of acetone. The chemical equation for that reaction is:


H2(g) + F2(g) → 2 HF(g)        ΔH°rxn = -540 kJ


This equation is balanced. 


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Problem Details

Gaseous hydrogen and fluorine combine in the reaction below to form hydrogen fluoride:

H2(g) + F2(g) → 2 HF(g)        ΔH°rxn = -540 kJ

What is the value of the heat of formation for HF(g)?

A) -1080 kJ/mol

B) -540 kJ/mol

C) -270 kJ/mol

D) 270 kJ/mol

E) 540 kJ/mol

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