Estimate the heat of combustion (in kJ) for propane, C₃H₈, using the following bond dissociation energies:

Consider the two reactions below: 

i) HBr(g) + H₂O(g) ↔ Br^-(g) + H₃O⁺(g) 

ii) HI(g) + H₂O(g) ↔ I^-(g) + H₃O⁺(g)

Calculate the enthalpies of reaction using bond enthalpies and identify if both reactions are exothermic or not.

The heat of atomization is defined as the enthalpy change that accompanies the total breakdown of a molecule into its constituent atoms (gas phase). The heat of atomization of SiH₄ is 1194 kJ/mol while it is 1351 kJ/mol for SiH₃Cl. Using only this data, calculate the bond energy for the Si—Cl bond.

The electrostatic potential map below corresponds to either propanol (C₃H₈O), propane (C₃H₈), chloropropane (C₃H₇Cl), or propanone (C₃H₆O). Which one is it?

The potential energy of two atoms as a function of internuclear distance is depicted in the diagram below. 

True or False. The repulsive forces between the two atoms are strongest at point B.

Calculate the  electrostatic force of attraction in N between a proton and electron that are separated by 1.32 nm

Shown below are six ions: A, B, C, X, Y, Z, with their charges and relative ionic radii. Which 1:1 ion combination has the lowest lattice energy?

MgO and CaS both adopt a similar crystal structure. The distance between cations and anions is the only distinction between the two. Estimate the Mg–O and the Ca–S distances. Use the following information:

Consider the following compounds: LiAt, CsBr, BaTe, MgSe. Sort the compounds from the lowest to the highest magnitude of lattice energy.

The lattice energy of CuCl₂(s) is 2824 kJ/mol. Use the Born-Haber cycle to determine the ΔH°_f for CuCl₂(s) from its elements. Compare this with the ΔH°_f for CuCl(s) (–137.2 kJ/mol) and determine which compound is more stable.

Using knowledge of the formation of KCl from its elements, construct a Born-Haber cycle for KCl.