Question

What is the estimated standard enthalpy of formation (ΔHf°) for magnesium fluoride (MgF₂) based on the given data?

A) -3469 kJ/mol

B) -2693 kJ/mol

C) -1821 kJ/mol

D) -4285 kJ/mol

Answer 1

The data provided is insufficient to accurately calculate the standard enthalpy of formation (∆Hf°) for magnesium fluoride (MgF₂). Normally, the calculation would be based on the standard enthalpies of formation of reactants and products and applying Hess's Law.

Step-by-step explanation:

To estimate the standard enthalpy of formation (∆Hf°) for magnesium fluoride (MgF₂), we must combine known enthalpies. However, the provided data appears to be incomplete and does not provide enough information to solve for the standard enthalpy of formation of MgF₂. Typically, you would use standard enthalpies of formation for the reactants and products, applying Hess's Law to find the overall enthalpy change for a reaction. In this case, we have a reference to a figure for the lattice energy for MgH₂ and the electron affinity for fluorine, but the data is not sufficient to calculate ∆Hf° for MgF₂.