Question 4 of 17 O Attempt 1 Consider the combustion reaction for octane (C,H3), which is a primary component of gasoline. 2 C3H18 + 25 O, 16 CO, + 18 H,O How many moles of CO, are emitted into the atmosphere when 13.6 g C, H, is burned? 1.90 CO, emitted: Incorrect 12:18 62°F 11/9/2 PC DELL
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.
![**Combustion Reaction of Octane (C₈H₁₈)**
Consider the combustion reaction for octane (\(C_8H_{18}\)), which is a primary component of gasoline:
\[
2\,C_8H_{18} + 25\,O_2 \rightarrow 16\,CO_2 + 18\,H_2O
\]
**Problem Statement:**
How many moles of \(CO_2\) are emitted into the atmosphere when 13.6 g of \(C_8H_{18}\) is burned?
**User Input:**
- CO₂ emitted: 1.90 moles
**Feedback:**
- Status: Incorrect
**Explanation:**
The problem requires calculating the moles of carbon dioxide produced when a given mass of octane is combusted. The balanced chemical equation indicates the stoichiometry of the reaction. Based on the molar relationship, 2 moles of \(C_8H_{18}\) produce 16 moles of \(CO_2\).
Follow-up calculations would involve finding the molar mass of \(C_8H_{18}\), converting the given mass (13.6 g) to moles, and using stoichiometry to determine the correct amount of \(CO_2\) produced.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3cec513c-d16e-482b-87a0-612878f683f9%2Fd6c3ea0d-41ef-4001-a9e8-1855941b56a2%2F0yneunb_processed.jpeg&w=3840&q=75)
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