All Chapters
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
Ch.8 - Periodic Properties of the Elements
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: Propane, C3H8, is a hydrocarbon that is commonly used as a fuel.Calculate the volume of air at 25°C and 1.00 atmosphere that is needed to completely combust 25.0 grams of propane. Assume that air is 2

Solution: Propane, C3H8, is a hydrocarbon that is commonly used as a fuel.Calculate the volume of air at 25°C and 1.00 atmosphere that is needed to completely combust 25.0 grams of propane. Assume that air is 2

Problem

Propane, C3H8, is a hydrocarbon that is commonly used as a fuel.

Calculate the volume of air at 25°C and 1.00 atmosphere that is needed to completely combust 25.0 grams of propane. Assume that air is 21.0 percent O2 by volume. (Hint: we will see how to do this calculation in a later chapter on gases—for now use the information that 1.00 L of air at 25°C and 1.00 atm contains 0.275 g of O2 per liter.)

Solution
  • Start by writing the balanced combustion reaction of propane. 
  • From the mass of propane, we can use the balanced equation to get the moles  of Oby stoichiometry
  • Moles of Owill be plugged into an ideal gas equation to find V of O2
  • V of air will be calculated from V of O2 using the information where 21% of air is made up of O2
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