2) Please determine the enthalpy for the following reaction using the enthalpies of the three reactions below. To receive full credit, describe or show how you manipulated each equation. Find the enthalpy for: 5C(s) + 6H2(g) → C;H12(1) Using these reactions: C5H12 (1) + 802(g) → 5C02(g) + 6H20(g) AHrxn = -3244.8 kJ C(s)+ 02(g) → CO2(g) AHrxn = -393.5 k] 2H2(g) + 02(g) → 2H20(g) AHrxn = -483.5 kJ
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.
![**Problem 2: Determining Reaction Enthalpy**
To find the enthalpy for the reaction:
\[ \text{5C(s)} + \text{6H}_2(g) \rightarrow \text{C}_5\text{H}_{12}(l) \]
Use the following reactions and their enthalpies:
1. \(\text{C}_5\text{H}_{12}(l) + 8\text{O}_2(g) \rightarrow 5\text{CO}_2(g) + 6\text{H}_2\text{O}(g)\), \(\Delta H_{\text{rxn}} = -3244.8 \, \text{kJ}\)
2. \(\text{C}(s) + \text{O}_2(g) \rightarrow \text{CO}_2(g)\), \(\Delta H_{\text{rxn}} = -393.5 \, \text{kJ}\)
3. \(2\text{H}_2(g) + \text{O}_2(g) \rightarrow 2\text{H}_2\text{O}(g)\), \(\Delta H_{\text{rxn}} = -483.5 \, \text{kJ}\)
**Solution Instructions:**
To calculate the enthalpy of the target reaction, you need to manipulate these given reactions, ensuring you balance and reverse equations as necessary to align with the target reaction steps. This involves considering the stoichiometry and potentially reversing reactions (which changes the sign of \(\Delta H\)) to achieve the desired result.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe4623fc6-165c-41ee-ad2c-ab19e78f0a44%2Fe2b91b4f-1dfe-4b74-abcd-b50bdfb92e67%2F0xsm6je_processed.png&w=3840&q=75)
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