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

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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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**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.
Transcribed Image Text:**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.
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