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: Calculate ΔH° (in kJ) for the reaction. 2S (s) + 3O2 (g) → 2SO3 (g)  ∆H = -790 kJ S (s) + O2 (g) → SO2 (g)        ∆H = -297 kJ the enthalpy of the reaction in which sulfur dioxide is oxidized to su

Problem

Calculate ΔH° (in kJ) for the reaction.

2S (s) + 3O2 (g) → 2SO3 (g)  ∆H = -790 kJ

S (s) + O2 (g) → SO2 (g)        ∆H = -297 kJ

the enthalpy of the reaction in which sulfur dioxide is oxidized to sulfur trioxide is ________ kJ.

 

a) -196

b) -543

c) 1087

d) 196

d) -1384