Q. Q. the ionization enthalphy for Na+ (g) formation from Na(g) is 495.8 kJ mol-1 ; while the electron gain enthalphy for the change Cl(g) + e -> Cl-(g) is , -348 kJ mol-1 only. The sum of the two, 147.1 kJ mol-1 is more than compensated for by the enthalphy of lattice formation of NaCl(s) (-788 kJ mol-1). Therefore, the energy released in the processes is more than the energy absorbed. But according to the data, Ionization enthalpy (energy absorbed) = 495.8 . It is greater than electron gain enthalpy (released) = -348.7. The energy absorbed is more than released.
Dear Student,
In the formation of NaCl from Na and Cl,
The process involved are- ionization of Na to form Na+ , gain of electron by Cl to form Cl-. Then the formation of lattice by the two ions.
From the given data we can see that,
the energy released during the reaction = electron gain enthalpy + enthalpy of lattice formation = -348.7 + (-788) kJ/mol = -1136.7kJ/mol
And the energy absorbed during the reaction = ionizaton enthalpy = 495.8kJ/mol.
It can now be clearly seen that the energy released is much more than of the energy absorbed.
Hope this information will clear your doubts about the topic. If you have any other doubt, just post it on the forum and our experts will help you out as soon as possible.
Regards,
In the formation of NaCl from Na and Cl,
The process involved are- ionization of Na to form Na+ , gain of electron by Cl to form Cl-. Then the formation of lattice by the two ions.
From the given data we can see that,
the energy released during the reaction = electron gain enthalpy + enthalpy of lattice formation = -348.7 + (-788) kJ/mol = -1136.7kJ/mol
And the energy absorbed during the reaction = ionizaton enthalpy = 495.8kJ/mol.
It can now be clearly seen that the energy released is much more than of the energy absorbed.
Hope this information will clear your doubts about the topic. If you have any other doubt, just post it on the forum and our experts will help you out as soon as possible.
Regards,