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: Use the standard reaction enthalpies given below to determine ΔH°rxn for the following reaction: 2S(s) + 3O2(g) → 2SO3(g)     ΔH°rxn = ? Given: SO2(g) → S(s) + O2(g)       ΔH°rxn = +296.8 kJ 2SO2(g) +

Solution: Use the standard reaction enthalpies given below to determine ΔH°rxn for the following reaction: 2S(s) + 3O2(g) → 2SO3(g)     ΔH°rxn = ? Given: SO2(g) → S(s) + O2(g)       ΔH°rxn = +296.8 kJ 2SO2(g) +

Problem

Use the standard reaction enthalpies given below to determine ΔH°rxn for the following reaction: 

2S(s) + 3O2(g) → 2SO3(g)     ΔH°rxn = ? 

Given: SO2(g) → S(s) + O2(g)       ΔH°rxn = +296.8 kJ 

2SO2(g) + O2(g) → 2SO3(g)       ΔH°rxn = -197.8 kJ 

a. -494.6 kJ 

b. -692.4 kJ 

c. -791.4 kJ 

d. -98.8 kJ 

e. -293.0 kJ

Solution

To find the ΔHrxn, we need to use the Hess's Law where we have to rearrange the given equations to get the desired reaction

View the complete written solution...