18. Use the chemical equations shown below to determine the enthalpy for the reaction: Fe,O«(s) + CO(g) – 3FEO(s) + CO:(g) AH° = ? (1) 2 Fe(s) + 3CO2(g) → Fe;O:(s) + 3 CO(g) AH,° (2) 3 Fe,O:(s) + CO(g) -2 Fe,O4(s) + CO:(g) (3) FeO(s) + CO(g) Fe(s) + CO:(g) AH;° AH,° O A) AH1° + AH2° + AH3° B) 3/2 ΔΗ'- 12 ΔΗ2ρό -3 ΔΗ5 C) - 3/2 AH1° - 1/2 AH2° - 3 AH3° D) - AH1° - 2 AH2° - 1/3 AH3° O E) 3/2 AH1° - 2 AH2° -3 AH3°
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.
![### Determining Enthalpy Change of a Reaction
#### Problem Statement
Use the chemical equations shown below to determine the enthalpy (\(\Delta H^\circ\)) for the reaction:
\[\text{Fe}_3\text{O}_4(s) + \text{CO}(g) \rightarrow 3\text{Fe}(s) + \text{CO}_2(g)\]
\[\Delta H^\circ =?\]
#### Given Chemical Equations
1. \(2 \text{Fe}(s) + 3\text{CO}_2(g) \rightarrow \text{Fe}_3\text{O}_4(s) + 3\text{CO}(g)\) \(\Delta H_1^\circ\)
2. \(3 \text{Fe}_3\text{O}_4(s) + \text{CO}(g) \rightarrow 2 \text{Fe}_2\text{O}_3(s) + \text{CO}_2(g)\) \(\Delta H_2^\circ\)
3. \(\text{FeO}(s) + \text{CO}(g) \rightarrow \text{Fe}(s) + \text{CO}_2(g)\) \(\Delta H_3^\circ\)
#### Multiple Choice Options
A) \(\Delta H_1^\circ + \Delta H_2^\circ + \Delta H_3^\circ\)
B) \(\frac{3}{2} \Delta H_1^\circ - \frac{1}{2} \Delta H_2^\circ - 3 \Delta H_3^\circ\)
C) \(- \frac{3}{2} \Delta H_1^\circ - \frac{1}{2} \Delta H_2^\circ - 3 \Delta H_3^\circ\)
D) \(- \Delta H_1^\circ - 2 \Delta H_2^\circ - \frac{1}{3} \Delta H_3^\circ\)
E) \(\frac{3}{2} \Delta H_1^\circ - 2 \Delta H_2^\circ - 3 \Delta H_3^\circ\)
### Explanation of the Graphs/Diagrams
This problem involves combining given enthalpies for a set of reactions to determine the enthalpy of the target](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fad75d3c3-f925-415c-aa85-2c90219f0688%2F5c19bd74-b9f4-4689-af58-9ce19d675f73%2Fy2h6rbu_processed.png&w=3840&q=75)
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