Determine the standard enthalpy of formation (AH°t) for NO2(g) given the information from the following reaction, where AH°† for N20(g) = + 82.1 kJ/mol. 2N20(g) + 302(g) → 4NO2(g) AHrxn = -31.4kJ
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 the Standard Enthalpy of Formation for NO₂(g)**
Given Reaction:
\[ \text{2N₂O(g) + 3O₂(g) → 4NO₂(g)} \]
- **ΔH°ₓᵢₙ** (Standard Enthalpy Change of Reaction) = -31.4 kJ
- **ΔH°f for N₂O(g)** = + 82.1 kJ/mol
**Explanation:**
This equation provides data to calculate the standard enthalpy of formation (ΔH°f) for NO₂(g) using the enthalpy change of the overall reaction and the given data for N₂O(g).
The enthalpy change for the reaction (ΔHₓᵢₙ) and the formation enthalpy of N₂O(g) are used to determine the formation enthalpy of NO₂(g), involving stoichiometry and thermodynamic calculations. No graph or diagram is present.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fbc3eda98-838a-48fa-9790-2f190fa845b2%2F13f2df78-7fbc-4e99-9aed-e2368203b294%2Fi2v9nyo_processed.png&w=3840&q=75)
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