Answer
The correct answers are:
a. ΔE = -419 kJ/mol
b. ΔE = -532 kJ/mol
c. ΔE = -718 kJ/mol
d. ΔE = -564 kJ/mol
Work Step by Step
To estimate the change in energy (ΔE) for the given reactions, we need to use the bond energies, electron affinities, and the ionization energy of hydrogen.
a. HF(g) → H⁺(g) + F⁻(g)
ΔE = Bond energy of H-F - Ionization energy of H - Electron affinity of F
ΔE = 565 kJ/mol + 1312 kJ/mol - 328 kJ/mol = 1549 kJ/mol
b. HCl(g) → H⁺(g) + Cl⁻(g)
ΔE = Bond energy of H-Cl - Ionization energy of H - Electron affinity of Cl
ΔE = 427 kJ/mol + 1312 kJ/mol - 349 kJ/mol =1390 kJ/mol
c. HI(g) → H⁺(g) + I⁻(g)
ΔE = Bond energy of H-I - Ionization energy of H - Electron affinity of I
ΔE = 295 kJ/mol + 1312 kJ/mol - 295 kJ/mol = 1312 kJ/mol
d. H₂O(g) → H⁺(g) + OH⁻(g)
ΔE = Bond energy of O-H) - Ionization energy of H - Electron affinity of OH
ΔE = (467 kJ/mol) + 1312 kJ/mol - 180 kJ/mol = 1599 kJ/mol
