contestada

Consider the following information. The lattice energy of CsCl is Δ H lattice = − 657 kJ/mol. The enthalpy of sublimation of Cs is Δ H sub = 76.5 kJ/mol. The first ionization energy of Cs is IE 1 = 376 kJ/mol. The electron affinity of Cl is Δ H EA = − 349 kJ/mol. The bond energy of Cl 2 is BE = 243 kJ/mol. Determine the enthalpy of formation, Δ H f , for CsCl ( s ) .

Respuesta :

IthaloAbreu

Answer:

-310.5 kJ/mol

Explanation:

The CsCl(s) will be formed by steps:

  • The metal (Cs) will be made gaseous by a sublimation → ΔHsub = 76.5 kJ/mol;
  • The metal gains energy to ionize → IE = 376 kJ/mol;
  • The nonmetal (Cl) loses energy to ionizes → EA = -349 kJ/mol;
  • The nonmetal is bonded → BE = 243 kJ/mol;
  • The lattice is formed → ΔHlattice = -657 kJ/mol.

The enthanlpy of formation is the sum of all the energies involved in the steps:

ΔHf = 76.5 + 376 -349 + 243 -657

ΔHf = -310.5 kJ/mol

pstnonsonjoku

The enthalpy of formation of CsCl is -311 kJ/mol.

We have the following information from the question;

Lattice energy ( ΔH lattice) = − 657 kJ/mol

Heat of sublimation of Cs ( ΔH sub) = 76.5 kJ/mol

Ionization energy of Cs (IE) =  376 kJ/mol

Bond energy of Cl2 (BE) = 243 kJ/mol

Electron affinity of C l(EA) = − 349 kJ/mol

Using Hess law of constant heat summation;

ΔHf(CsCl) =    ΔH sub + BE+ IE + EA + ΔH lattice

ΔHf(CsCl) = 76.5 kJ/mol + 243 kJ/mol + 376 kJ/mol + (− 349 kJ/mol) (− 657 kJ/mol)

ΔHf(CsCl) = -311 kJ/mol

Learn more: https://brainly.com/question/18956703

Otras preguntas