Final answer:
The iron and chlorine reaction forms iron(II) chloride, and by using the given information and calculating the moles of Fe involved, the enthalpy change for 1 mole of FeCl2 can be determined.
Step-by-step explanation:
When iron combines with chlorine gas, it forms an ionic compound called iron(II) chloride. This reaction can be represented by the chemical equation: Fe(s) + Cl2(g) → FeCl2(s). To calculate the enthalpy change for the reaction when 1 mole of FeCl2(s) is produced, we can use the given reaction data.
First, we need to determine the moles of Fe used in the reaction using its molar mass (55.845 g/mol). With 1.42 g of iron used, we calculate the moles of Fe and then apply the known heat production to find the enthalpy change for one mole of FeCl2.
Steps to calculate the enthalpy change:
Determine moles of Fe: Moles = mass (g) / molar mass (g/mol).
Use the ratio of moles of Fe to moles of FeCl2 formed.
Calculate the enthalpy change (ΔH) per mole of FeCl2 using the formula: ΔH = (q of the reaction in kJ) / moles of FeCl2.
As per the given information, 1.42 g of Fe reacts to give 8.60 kJ of heat. Therefore, using Fe's molar mass: Moles of Fe = 1.42 g / 55.845 g/mol, we get the moles of Fe which then relate to moles of FeCl2. Finally, we can calculate the enthalpy change for the reaction when 1 mole of FeCl2(s) is produced.