Given the following reactions: Rxn Reaction AG° (kJ) #: 1) N2 (g) + 3 H2 (g) → 2 NH3 (g) -32.0 2) N2 (g) + 4 H2 (g) + Cl2 (g)→ 2 NH4CI (s) + Cl2 (e) → 2 NH4CI (s) -406.0 3) NH3 (g) + HCI (g) → NH4CI (s) -91.7 use a process similar to Hess's Law to calculate the AG°Rxn for the following reaction: Overall: H2 (e) + Cl2 (g) → 2 HCI (g) (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.
All boxes please.
box 1 answer choices: reverse or forward.
box 2 answer choices: 2, -1/2, -2, 1, 1/2, or -1.
box 3 answer choices: reverse or forward.
box 4 answer choices: 2, -2, 1/2, -1, -1/2, or 1.
box 5 answer choices: forward or reverse.
box 6 answer choices: 2, -2, 1, 1/2, -1/2, or -1.
box 7 answer choices: -557.4, 621.4, 381.2, -529.7, -381.2, -282.3, -621.4, -190.6, -254.6, 529.7, or 282.3.
box 8 answer choices: -95.3, 381.2, -381.2, 264.9, -264.9, -141.2, 95.3, or 141.2.
![**Title: Analysis of ΔG° in Chemical Reactions**
---
**Section: Reaction Parameters**
- **Reaction 2:**
- **Direction:** [Select]
- **Multiplier on ΔG° (including sign):** [Select]
- **Reaction 3:**
- **Direction:** [Select]
- **Multiplier on ΔG° (including sign):** [Select]
**Section: Calculating Overall Reaction Conditions**
- **b) What is the ΔG°<sub>Rxn</sub> for the overall reaction as written?**
- [Select]
- **c) What is this value per mole of HCl?**
- [Select]
---
**Graph/Diagram Explanation:**
This section presents dropdown menus for selecting parameters determining the direction and the multiplier on the standard change in free energy (ΔG°) for reactions. The information will be used to calculate the Gibbs free energy for the overall reaction and determine the corresponding value per mole of HCl.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F96529d31-1af4-4d90-b6c1-79b0ae971a1c%2F0aca5ee8-3fb9-4997-a5ba-ce001d8cc70e%2F794xow_processed.png&w=3840&q=75)
![Given the following reactions:
| Rxn # | Reaction | ΔG° (kJ) |
|-------|----------------------------------------|----------|
| 1 | \( \text{N}_2(g) + 3 \text{H}_2(g) \rightarrow 2 \text{NH}_3(g) \) | -32.0 |
| 2 | \( \text{N}_2(g) + 4 \text{H}_2(g) + \text{Cl}_2(g) \rightarrow 2 \text{NH}_4\text{Cl}(s) \) | -406.0 |
| 3 | \( \text{NH}_3(g) + \text{HCl}(g) \rightarrow \text{NH}_4\text{Cl}(s) \) | -91.7 |
Use a process similar to Hess's Law to calculate the \( \Delta G^\circ_{\text{Rxn}} \) for the following reaction:
**Overall:**
\[ \text{H}_2(g) + \text{Cl}_2(g) \rightarrow 2 \text{HCl}(g) \]
And answer the following questions:
a) For each of the given reactions, choose the direction and the multiplier on ΔG° (including the sign if negative).
**Reaction 1:**
- **Direction:** [Select]
- **Multiplier on ΔG° (including sign):** [Select]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F96529d31-1af4-4d90-b6c1-79b0ae971a1c%2F0aca5ee8-3fb9-4997-a5ba-ce001d8cc70e%2Fazthbf_processed.png&w=3840&q=75)
Step by step
Solved in 6 steps
