The following are various δ H values (kJ per mol): delta_f H() = -411.2; delta_sub H(Na, g) = 107.3; delta_i H(Na, g) = 495.4; delta_eg H(Cl, g) = -348.5. The Lattice enthalpy of (s) is

Question

The following are various δ H values (kJ per mol): delta_f H($NaCl$) = -411.2; delta_sub H(Na, g) = 107.3; delta_i H(Na, g) = 495.4; delta_eg H(Cl, g) = -348.5. The Lattice enthalpy of $NaCl$(s) is

Prashant Kotian · Accepted Answer

Correct answer: D. Born-Haber: U_Lattice = sub_H(Na) + IE(Na) + atomization_H(Cl) + EA(Cl) - delta_f H() = 107.3 + 495.4 + 121.7 - 348.5 - (-411.2) = 787.1 kJ/mol.

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