Answer:
ΔH for 1 mole of FeCl2 is -338.58 kJ/mol
Explanation:
Step 1: Data given
Mass of iron = 1.42 grams
Mass of chlorine = 1.80 grams
Mass of FeCl2 = 3.22 grams
Heat produced = 8.60 kJ (ΔH = -8.60 kJ because the reaction is exothermic)
Molar mass of Fe = 55.845 g/mol
Molar mass of Cl2 = 70.9 g/mol
Molar mass of FeCl2 = 126.75 g/mol
Step 2: The balanced equation
Fe + Cl2 → FeCl2
Step 3: Calculate moles of FeCl2
Moles FeCl2 = Mass FeCl2 / Molar mass FeCL2
Moles FeCl2 = 3.22 grams / 126.75 g/mol
Moles FeCl2 = 0.0254 moles
Step 4: Calculate the enthalpy change for 1 mole of FeCl2
For 0.0254 moles of FeCl2 ΔH is -8.60 kJ
For 1 mole of FeCL2 ΔH = -8.60 / 0.0254mol = -338.58 kJ/mol
ΔH for 1 mole of FeCl2 is -338.58 kJ/mol
