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Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
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Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: The combustion of octane, C8H18, proceeds according to the reaction2C8H18(l) + 25O2(g) → 16CO2(g) + 18H2O(l) If 305 mol of octane combusts, what volume of carbon dioxide is produced at 35.0°C and 0.995 atm?

Solution: The combustion of octane, C8H18, proceeds according to the reaction2C8H18(l) + 25O2(g) → 16CO2(g) + 18H2O(l) If 305 mol of octane combusts, what volume of carbon dioxide is produced at 35.0°C and 0.99

Problem

The combustion of octane, C8H18, proceeds according to the reaction

2C8H18(l) + 25O2(g) → 16CO2(g) + 18H2O(l) 

If 305 mol of octane combusts, what volume of carbon dioxide is produced at 35.0°C and 0.995 atm?


Solution

We are asked to calculate the volume of carbon dioxide (CO2) produced from the combustion of octane (C8H18). We can calculate the volume of the gas using the ideal gas equation:

P = pressure, atm
 V = volume, L
 n = moles, mol
 R = gas constant = 0.08206 (L·atm)/(mol·K)
 T = temperature, K


In the ideal gas equation, the amount of CO2 in moles is needed but the moles of C8H18 is given instead. We will have to calculate the moles of CO2 produced from CH4 first using the balanced reaction equation and mole to mole comparison.

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