A chemist measures the enthalpy change AH during the following reaction: CH₁2O6(s) 3 CH4(9) + 3 CO₂(9) ΔΗ=-132, kJ Use this information to complete the table below. Round each of your answers to the nearest kJ. reaction 3C H₁20 (s) 9CH, (g) + 9C0₂(g) ẾCH,) +=CO,) + ẾCH,,0,0) 3CH₂(g) + 3C0₂(g) → CH₁₂O(s) AH 1kJ kJ X 3
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.
![### Understanding Enthalpy Change (ΔH) in Chemical Reactions
A chemist measures the enthalpy change (ΔH) during the following reaction:
\[ \text{C}_6\text{H}_{12}\text{O}_6(s) \rightarrow 3 \text{CH}_4(g) + 3 \text{CO}_2(g) \]
The enthalpy change for this reaction is:
\[ ΔH = -132 \text{ kJ} \]
This value signifies the energy change involved in the reaction, with the negative sign indicating that energy is released, making the reaction exothermic.
### Completing the Table
Use the information above to determine the enthalpy changes for the reactions listed in the table below. Round your answers to the nearest kJ.
| Reaction | ΔH |
|----------|----|
| \( 3\text{C}_6\text{H}_{12}\text{O}_6(s) \rightarrow 9\text{CH}_4(g) + 9\text{CO}_2(g) \) | □ kJ |
| \( \frac{1}{2} \text{CH}_4(g) + \frac{1}{2} \text{CO}_2(g) \rightarrow \frac{1}{6} \text{C}_6\text{H}_{12}\text{O}_6(s) \) | □ kJ |
| \( 3\text{CH}_4(g) + 3\text{CO}_2(g) \rightarrow \text{C}_6\text{H}_{12}\text{O}_6(s) \) | □ kJ |
### Explanation
- The first reaction is a scaled-up version of the given reaction by a factor of three.
- The second and third reactions involve reverse processes with adjustments in the stoichiometry to represent half-reactions or reversed reactions.
- Completing this exercise requires understanding of stoichiometry and the manipulation of enthalpy in chemical equations, such as multiplying or dividing by constants. Adjustments reflect the given enthalpy change of the initial reaction.
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