Substance CO(g) O₂(g) CO₂(g) c. d. 1.22 x 1045 8.23 x 10-46 e. 7.48 x 1068 AHfᵒ (kJ/mol) ? 0 -393.5 CO(g) + ¹102(g) ⇒ CO₂(g) AH° = -283.0 kJ/mol 11) What is the value of K for the reaction showing the production of CO₂(g) at 298K? a. 1.05 x 10-69 b. 1.11 x 1024 12) What is the AS° for the reaction at 298K? a. -86.6 J/mol-K b. -118 J/mol-K d. c. -16.0 J/mol-K -189 J/mol-K e. -300 l/mol-K AGfᵒ (kJ/mol) -137.2 0 -394.4 Sº (J/mol-K) 197.7 205.1 213.7
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.
![**Thermodynamic Properties and Reaction Calculations**
The table below lists thermodynamic properties of substances involved in a specific chemical reaction:
| Substance | ΔHf° (kJ/mol) | ΔGf° (kJ/mol) | S° (J/mol-K) |
|-----------|--------------|--------------|-------------|
| CO(g) | ? | -137.2 | 197.7 |
| O2(g) | 0 | 0 | 205.1 |
| CO2(g) | -393.5 | -394.4 | 213.7 |
**Reaction:**
\[ \text{CO(g) + ½O}_2\text{(g) ⇌ CO}_2\text{(g)} \]
ΔH° = -283.0 kJ/mol
**Questions:**
**11) What is the value of K for the reaction showing the production of CO\(_2\)(g) at 298K?**
a. \(1.05 \times 10^{-69}\)
b. \(1.11 \times 10^{24}\)
c. \(1.22 \times 10^{45}\)
d. \(8.23 \times 10^{-46}\)
e. \(7.48 \times 10^{68}\)
**12) What is the ΔS° for the reaction at 298K?**
a. \(-86.6 \text{ J/mol-K}\)
b. \(-118 \text{ J/mol-K}\)
c. \(-16.0 \text{ J/mol-K}\)
d. \(-189 \text{ J/mol-K}\)
e. \(-300 \text{ J/mol-K}\)
**Explanation for Graphs or Diagrams:**
In this problem set, no graphs or diagrams are present. The data provided is in tabular form detailing the thermodynamic properties of CO, O2, and CO2. The focus is on calculating equilibrium constants and entropy change for the given reaction using the provided thermodynamic data.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2a7b7893-fc75-4209-832c-2d35b2c13ae8%2Fa14ed1c0-fba3-48d8-8cd3-bde254f90c5b%2F52g71ii_processed.png&w=3840&q=75)
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