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
Sections
Internal Energy
Calorimetry
Hess's Law
Enthalpy of Formation
End of Chapter 6 Problems
Additional Practice
Units of Energy
Endothermic & Exothermic Reactions
Additional Guides
Enthalpy

Solution: From the enthalpies of reactionH2 (g) + F2 (g) → 2 HF (g)          ΔH = -537 kJC (s) + 2 F2 (g) → CF4 (g)          ΔH = -680 kJ2 C (s) + 2 H2 (g) → C2H4 (g)     ΔH = +52.3 kJcalculate ΔH for the reaction of ethylene with F 2:C2H4 (g) + 6 F2 (g) → 2 CF4 (g) + 4 HF (g) 

Problem

From the enthalpies of reaction
H2 (g) + F2 (g) → 2 HF (g)          ΔH = -537 kJ
C (s) + 2 F2 (g) → CF4 (g)          ΔH = -680 kJ
2 C (s) + 2 H2 (g) → C2H4 (g)     ΔH = +52.3 kJ

calculate ΔH for the reaction of ethylene with F 2:
C2H4 (g) + 6 F2 (g) → 2 CF4 (g) + 4 HF (g)