What mass of water will be produced from the combustion of 1 gallon of octane (C3H18) given that the density of octane is 0.79 g/mL? (1 gallon = 3.8 L) %3D
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.
![**Question 3 of 8**
**Transcription for Educational Website:**
**Combustion of Octane and Water Production**
What mass of water will be produced from the combustion of 1 gallon of octane (C₈H₁₈) given that the density of octane is 0.79 g/mL? (1 gallon = 3.8 L)
**Explanation:**
To solve this problem, you need to follow these steps:
1. **Convert gallons to liters:**
- 1 gallon = 3.8 liters
2. **Calculate the mass of octane:**
- Density formula: Density = Mass/Volume
- Mass = Density × Volume
- Volume of octane = 3.8 L = 3800 mL (since 1 L = 1000 mL)
- Mass of octane = 0.79 g/mL × 3800 mL
3. **Use stoichiometry to find the mass of water:**
- Balanced chemical equation for the combustion of octane:
\[
2C_8H_{18} + 25O_2 \rightarrow 16CO_2 + 18H_2O
\]
- According to the equation, 2 moles of octane produce 18 moles of water.
4. **Calculate moles of octane:**
- Molar mass of C₈H₁₈ = (8×12.01) + (18×1.01) = 114.22 g/mol
- Moles of octane = Mass of octane / Molar mass of C₈H₁₈
5. **Calculate moles of water produced:**
- Use the stoichiometric ratio from the balanced equation.
6. **Convert moles of water to grams:**
- Molar mass of H₂O = 18.02 g/mol
- Mass of water = Moles of water × Molar mass of H₂O
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