Using standard heats of formation, calculate the standard enthalpy change for the following reaction. ΔΗ° rxn 2CO2 (g) + 5H2(g) → C₂H₂(g) + 4H₂O(g) AH (CO₂(g)) = -393.5 kJ/mol AH (H₂(g)) = 0.0 kJ/mol AH (C₂H₂ (9)) = 226.7 kJ/mol AH (H₂O(g)) kJ = - 241.8 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.
![**Using Standard Heats of Formation to Calculate Enthalpy Change**
To find the standard enthalpy change (\(\Delta H^\circ_{\text{rxn}}\)) for the reaction:
\[
2\text{CO}_2(g) + 5\text{H}_2(g) \rightarrow \text{C}_2\text{H}_2(g) + 4\text{H}_2\text{O}(g)
\]
we use the following standard heats of formation (\(\Delta H^\circ_f\)):
- \(\Delta H^\circ_f(\text{CO}_2(g)) = -393.5 \, \text{kJ/mol}\)
- \(\Delta H^\circ_f(\text{H}_2(g)) = 0.0 \, \text{kJ/mol}\)
- \(\Delta H^\circ_f(\text{C}_2\text{H}_2(g)) = 226.7 \, \text{kJ/mol}\)
- \(\Delta H^\circ_f(\text{H}_2\text{O}(g)) = -241.8 \, \text{kJ/mol}\)
**Calculate the standard enthalpy of the reaction:**
\[
\Delta H^\circ_{\text{rxn}} = \left( \sum \Delta H^\circ_f \text{(products)} \right) - \left( \sum \Delta H^\circ_f \text{(reactants)} \right)
\]
Using the above formula, determine the total \(\Delta H^\circ_{\text{rxn}}\).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4295bf62-da14-49f1-b3bf-6e678bc68de3%2Fca1f3f75-95a5-4803-bca5-9902b6583e01%2Fd6j2ue_processed.jpeg&w=3840&q=75)
![A scientist measures the standard enthalpy change for the following reaction to be -1122.6 kJ:
\[ 2\text{H}_2\text{S}(g) + 3\text{O}_2(g) \rightarrow 2\text{H}_2\text{O}(l) + 2\text{SO}_2(g) \]
Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of \(\text{H}_2\text{S}(g)\) is ____ kJ/mol.
| Species | \(\Delta H_f^\circ\) (kJ/mol) |
|---------|---------------------------|
| \(\text{H}_2\text{O}(l)\) | -285.8 |
| \(\text{SO}_2(g)\) | -296.8 |
| \(\text{O}_2(g)\) | 0.0 |](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4295bf62-da14-49f1-b3bf-6e678bc68de3%2Fca1f3f75-95a5-4803-bca5-9902b6583e01%2Fvpqhkm_processed.jpeg&w=3840&q=75)
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