Ch.6 - Thermochemistry WorksheetSee all chapters
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: Suppose you had a bomb calorimeter containing 500 mL of water at 25°C that you wanted to heat to exactly 95°C. You are using as a fuel the saturated fatty acid hexanedecanioc acid (C16H32O2), more commonly known as palmitic acid found in palm oil and animal fats. Use the following information to calculate how many grams of palmitic acid you should place into the bomb.Cbomb = 900 J/°C Cwater = 4.184 J/g°C density of water = 1.0 g/mL ΔHC-16.0 = 10, 071 kJ/mol (Heat of combustion of palmitic acid, assume ΔH = ΔE)

Problem

Suppose you had a bomb calorimeter containing 500 mL of water at 25°C that you wanted to heat to exactly 95°C. You are using as a fuel the saturated fatty acid hexanedecanioc acid (C16H32O2), more commonly known as palmitic acid found in palm oil and animal fats. 

Use the following information to calculate how many grams of palmitic acid you should place into the bomb.
Cbomb = 900 J/°C 

Cwater = 4.184 J/g°C 

density of water = 1.0 g/mL 

ΔHC-16.0 = 10, 071 kJ/mol (Heat of combustion of palmitic acid, assume ΔH = ΔE)