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: The combustion reaction of butane is as follows. C4H10(g) + 13/2 O2(g) → 4 CO2(g) + 5 H2O(l) Using Hess's law and the reaction enthalpies given below, find the change in enthalpy for this reaction. re

Solution: The combustion reaction of butane is as follows. C4H10(g) + 13/2 O2(g) → 4 CO2(g) + 5 H2O(l) Using Hess's law and the reaction enthalpies given below, find the change in enthalpy for this reaction. re

Problem

The combustion reaction of butane is as follows. 

C4H10(g) + 13/2 O2(g) → 4 CO2(g) + 5 H2O(l) 

Using Hess's law and the reaction enthalpies given below, find the change in enthalpy for this reaction. 

reaction (1):    C(s) + O2(g) → CO2(g)                               ΔH = -393.5 kJ/mol 

reaction (2):   H2(g) + 1/2 O2(g) → H2O(I)                        ΔH = -285.8 kJ/mol 

reaction (3):   4C(s) + 5H2(g) → C4H10 (g)                       ΔH = -125.7 kJ/mol