Similar to For practice 6.12)In the reaction shown here, 955 mL of O₂ forms at P = 0.950 atm and T-308 K. H s of Ag2O (molar mass = 231.8 g/mol) decomposed? O(s) --> 4 Ag(s) + O2(g) 15 g 574 g
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.
![### Problem Description:
**(6.7: Similar to For practice 6.12)** In the reaction shown here, 955 mL of O₂ forms at P = 0.950 atm and T = 308 K. How many grams of Ag₂O (molar mass = 231.8 g/mol) decomposed?
\[ 2Ag_2O(s) \rightarrow 4Ag(s) + O_2(g) \]
### Possible Answers:
- **☐ 1.15 g**
- **☐ 0.574 g**
- **☐ 8.32 g**
- **☐ 16.6 g**
### Solution Steps:
1. **Calculate the moles of O₂ formed** using the Ideal Gas Law equation PV = nRT, where:
- P = 0.950 atm
- V = 955 mL = 0.955 L (Note: 1 L = 1000 mL)
- T = 308 K
- R = 0.0821 L·atm/K·mol (Ideal Gas Constant)
Rearrange to find \( n \) (number of moles of O₂):
\[ n = \frac{PV}{RT} \]
2. **Use stoichiometry to relate moles of O₂ to moles of Ag₂O**. According to the balanced chemical equation:
\[ 2Ag_2O(s) \rightarrow 4Ag(s) + O_2(g) \]
- 1 mole of O₂ is produced from 2 moles of Ag₂O.
3. **Calculate the mass of Ag₂O needed**.
- Use the molar mass of Ag₂O (231.8 g/mol) and the number of moles of Ag₂O found in the stoichiometry step.
### Detailed Explanations:
- **Graphs/Diagrams**: There are no graphs or diagrams in this problem.
### Educational Objective:
The goal is to teach students how to use the Ideal Gas Law in combination with stoichiometry to solve for the mass of a reactant in a chemical reaction.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa6aa13af-b0b4-4b84-a222-8b6a152716db%2F19e23225-356f-4de7-ab03-6ddbe56223b7%2Fnojte_processed.jpeg&w=3840&q=75)
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