Use the following data to estimate AH for sodium chloride. Lattice energy Ionization energy for Na Electron affinity of C Bond energy of Cl₂ Enthalpy of sublimation for Na ΔΗ 1 Na(s) + Cl₂(g) → NaCl(s) 11 kJ/mol 787 kJ/mol 495 kJ/mol 349 kJ/mol 239 kJ/mol 109 kJ/mol
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
![**Estimating the Standard Enthalpy of Formation for Sodium Chloride**
To calculate the standard enthalpy of formation (\(\Delta H_f^\circ\)) for sodium chloride, use the following reaction and data:
\[ \text{Na(s)} + \frac{1}{2} \text{Cl}_2(g) \rightarrow \text{NaCl(s)} \]
**Given Data:**
- **Lattice Energy:** 787 kJ/mol
- **Ionization Energy for Na:** 495 kJ/mol
- **Electron Affinity of Cl:** -349 kJ/mol
- **Bond Energy of Cl\(_2\):** 239 kJ/mol
- **Enthalpy of Sublimation for Na:** 109 kJ/mol
**Formula:**
To estimate \(\Delta H_f^\circ\), combine these values using Hess's Law, considering the necessary steps to form sodium chloride from its elements.
**Calculation:**
\[
\Delta H_f^\circ = \text{sum of the energy changes}
\]
Fill in the calculated value in the blank provided:
\[ \Delta H_f^\circ = \boxed{\phantom{0}} \text{kJ/mol} \]
This approach uses known energy values to determine the overall energy change for the reaction forming NaCl from Na(s) and \(\frac{1}{2}\) Cl\(_2\)(g).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4cb3c08b-867c-49fa-a9fe-3ee9eddee973%2F9fafe84d-d45e-444d-ac7e-1475f0b65356%2Fzxl6zcb_processed.png&w=3840&q=75)
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