Calculate the Gºrxn using the following information. AHᵒf (kJ/mol) S°(J/mol*K) 4 HNO3(g) +5 N₂H4(l) → 7 N2(g) + 12 H₂O(1) -133.9 50.6 -285.8 266.9 121.2 70.0 +4.90 x 10³ kJ O +3.90 x 10³ kJ -2.04 x 103 kJ -3.15 x 10³ kJ -3.30 x 10³ kJ 191.6 AG rxn =?
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.
![**Title: Calculating ΔG° for a Reaction**
**Instructions:**
To determine the standard Gibbs free energy change (ΔG°) for the reaction below, utilize the given information about standard enthalpy of formation (ΔH°f) and standard entropy (S°).
**Reaction:**
\[ 4 \text{HNO}_3(g) + 5 \text{N}_2\text{H}_4(l) \rightarrow 7 \text{N}_2(g) + 12 \text{H}_2\text{O}(l) \]
**Data Table:**
| Substance | ΔH°f (kJ/mol) | S° (J/mol·K) |
|-----------|---------------|--------------|
| HNO₃(g) | -133.9 | 266.9 |
| N₂H₄(l) | 50.6 | 121.2 |
| N₂(g) | 0.0 | 191.6 |
| H₂O(l) | -285.8 | 70.0 |
**Question:**
Calculate ΔG°rxn for the reaction.
**Options:**
- ○ +4.90 x 10³ kJ
- ● +3.90 x 10³ kJ
- ○ -2.04 x 10³ kJ
- ○ -3.15 x 10³ kJ
- ○ -3.30 x 10³ kJ
**Note:**
The highlighted option is +3.90 x 10³ kJ, indicating the selected answer in the context.
To compute ΔG°, consider using the relationship:
\[ \Delta G^\circ = \Delta H^\circ - T \Delta S^\circ \]
Calculate using the provided standard values, assuming a specific temperature, typically 298 K (25 °C) unless stated otherwise.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb5cb748f-b247-416f-8df5-751d92c52687%2F920c75bf-0488-4476-96b3-b3d7c53cb558%2Fixjdeyk_processed.png&w=3840&q=75)
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