Question

Calculate ∆ᴏ, in kJ for this similar reaction below using ∆ᴏ data from section 12 of the data booklet.

∆ᴏ of HOCH₂CH₂OH(l) is -454.8kJ mol-1

Answer 1

To determine the ΔH° for a reaction with HOCH₂CH₂OH (l), use Hess's Law and the provided enthalpy data, which in this case is -454.8 kJ/mol for the given compound.

Step-by-step explanation:

To calculate the standard enthalpy change (ΔH°) for the reaction involving HOCH₂CH₂OH (l), we need to apply Hess's Law. Using the provided data, to find the enthalpy change for the unknown reaction, we generally sum the enthalpies of formation (ΔHⁿ) for the products and subtract the sum of the enthalpies of formation for the reactants. In this example, however, we are only given the enthalpy change of the compound of interest, HOCH₂CH₂OH (l), which is -454.8 kJ/mol. If that was the sole product or reactant, and we were depending on its given enthalpy change and the enthalpies of other species involved, we could plug those values into Hess's Law equation to find the standard enthalpy change for the reaction.