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 following data to calculate the standard heat (enthalpy) of formation, ΔH °f, of manganese(IV) oxide, MnO2 (s). 2MnO(s) → 2MnO (s) + O2 (g)          ΔH = 264 kJ MnO2 (s) + Mn(s) → 2MnO (s)           ΔH = -240 kJ Select one:(a) -504 kJ (b) -372 kJ (c) 24 kJ (d) -24 kJ (e) 504 kJ

Solution: Use the following data to calculate the standard heat (enthalpy) of formation, ΔH °f, of manganese(IV) oxide, MnO2 (s). 2MnO2 (s) → 2MnO (s) + O2 (g)          ΔH = 264 kJ MnO2 (s) + Mn(s) → 2MnO (s) 

Problem

Use the following data to calculate the standard heat (enthalpy) of formation, ΔH °f, of manganese(IV) oxide, MnO2 (s). 

2MnO(s) → 2MnO (s) + O2 (g)          ΔH = 264 kJ 

MnO2 (s) + Mn(s) → 2MnO (s)           ΔH = -240 kJ 

Select one:

(a) -504 kJ 

(b) -372 kJ 

(c) 24 kJ 

(d) -24 kJ 

(e) 504 kJ


Solution BlurView Complete Written Solution