Given the table of data below, what is the standard heat of reaction for the following process in klimo? Note that this reaction does not readily occur in the laboratory or in nature and the table provides more information than you actually need CH (9) H₂0 () CH₂O(g) + 2 H₂(g) Compound CH₂(g) H₂O(0) H₂O₂) 9106 HOOCHI CH,OH AH? (mol) -74.6 -285.8 -187.8 -115.9 -425.5 -2392
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.
![**Standard Heat of Reaction Calculation**
Given the table of data below, what is the standard heat of reaction for the following process in kJ/mol? Note that this reaction does not readily occur in the laboratory or in nature and the table provides more information than you actually need.
\[ \text{CH}_4 (g) + \text{H}_2\text{O} (l) \rightarrow \text{CH}_2\text{O} (g) + 2 \text{H}_2 (g) \]
### Compound and Standard Enthalpy of Formation (ΔHf in kJ/mol)
| Compound | ΔHf (kJ/mol) |
|----------|--------------|
| CH4 (g) | -74.8 |
| H2O (l) | -285.8 |
| H2O (g) | -187.8 |
| CH2O (g) | -115.9 |
| HCOOH (l) | -425.5 |
| CH3OH (l) | -239.2 |
### Options for Standard Heat of Reaction (ΔHr in kJ/mol)
- \( -115.9 \)
- \( -425.5 \)
- \( -220.7 \)
- \( -244.5 \)
- \( 220.7 \)
To calculate the standard heat of reaction (ΔHr), use the formula:
\[ \Delta H_r = \sum \Delta H_f(\text{products}) - \sum \Delta H_f(\text{reactants}) \]
*Substitute the values from the table into the equation to find the standard heat of the reaction.*
### Explanation of Table and Process
The table lists various compounds along with their standard enthalpy of formation (ΔHf in kJ/mol). When calculating the standard heat of reaction, it's essential to use the enthalpy values for products and reactants correctly.
- **Reactants:**
- \( \text{CH}_4 (g) \) with ΔHf = -74.8 kJ/mol
- \( \text{H}_2\text{O} (l) \) with ΔHf = -285.8 kJ/mol
- **Products:**
- \( \text{CH}_2\text{O} (g) \) with ΔHf](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F91caee7e-a450-4823-b604-91c802978c64%2F33b6b3f4-dcd1-4401-a217-00a766dbe5eb%2Ffsrhg2_processed.jpeg&w=3840&q=75)

Step by step
Solved in 3 steps with 3 images









