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: Data: ΔHf values: CH4 (g), -74.8 kJ: CO2 (g), -393.5 kJ: H2O (l), -285.8 kJ. Using the ΔHf data above, calculate ΔHrxn for the reaction below. Reaction: CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O (l) a. -604.2 kJ b. 8.90.3 kJ c. -997.7 kJ d. -890.3 kJ e. none of the above

Problem

Data: ΔHf values: CH4 (g), -74.8 kJ: CO2 (g), -393.5 kJ: H2O (l), -285.8 kJ. 

Using the ΔHf data above, calculate ΔHrxn for the reaction below. 

Reaction: CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O (l) 

a. -604.2 kJ 

b. 8.90.3 kJ 

c. -997.7 kJ 

d. -890.3 kJ 

e. none of the above