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: Given the following data: N2(g) + O2(g) → 2NO(g),          ΔH = +180.7 kJ 2NO(g) + O2(g) → 2NO2(g),     ΔH = -113.1 kJ 2N2O(g) → 2N2(g) + O2(g),      ΔH = -163.2 kJ Use Hess's law to calculate ΔH for the following reaction: N2O(g) + NO2(g) → 3NO(g) Express the enthalpy in kilojoules to four significant digits. 

Solution: Given the following data: N2(g) + O2(g) → 2NO(g),          ΔH = +180.7 kJ 2NO(g) + O2(g) → 2NO2(g),     ΔH = -113.1 kJ 2N2O(g) → 2N2(g) + O2(g),      ΔH = -163.2 kJ Use Hess's law to calculate ΔH for

Problem

Given the following data: 

N2(g) + O2(g) → 2NO(g),          ΔH = +180.7 kJ 

2NO(g) + O2(g) → 2NO2(g),     ΔH = -113.1 kJ 

2N2O(g) → 2N2(g) + O2(g),      ΔH = -163.2 kJ 

Use Hess's law to calculate ΔH for the following reaction: 

N2O(g) + NO2(g) → 3NO(g) 

Express the enthalpy in kilojoules to four significant digits. 


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