Combustion of octane (regular gasoline): 2 CaH18 + 25 02 → 16 CO2 + 18 H20 How many grams of CO2 are produced from burning 2.0 x 10³ grams of octane.
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 of Octane (Regular Gasoline):**
\[ 2 \text{C}_8\text{H}_{18} + 25 \text{O}_2 \rightarrow 16 \text{CO}_2 + 18 \text{H}_2\text{O} \]
**Question:**
How many grams of \(\text{CO}_2\) are produced from burning \(2.0 \times 10^3\) grams of octane?
**What is the 3rd step you would take?**
- **A:** Take grams of octane and divide by molar mass of carbon dioxide.
- **B:** Take moles of carbon dioxide and multiply by the molar mass of carbon dioxide to get grams of carbon dioxide.
- **C:** Convert moles of octane to moles of carbon dioxide using the molar ratio.
- **D:** Take grams of carbon dioxide and multiply by the molar mass of carbon dioxide to get moles of carbon dioxide.
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First, calculate the moles of octane by using the formula:
No of moles = Mass/Molar mass = (2.0×103g)/(114.23gmol-1) = 17.5 moles
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