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 oxidation of copper (l) oxide, Cu 2O(s), to copper(II) oxide, CuO(s), is an exothermic process, 2Cu2O(s) + O2(g) → 4CuO(s)                    ΔH°rxn = -292.0 kJ/mol Calculate the energy released a

Solution: The oxidation of copper (l) oxide, Cu 2O(s), to copper(II) oxide, CuO(s), is an exothermic process, 2Cu2O(s) + O2(g) → 4CuO(s)                    ΔH°rxn = -292.0 kJ/mol Calculate the energy released a

Problem

The oxidation of copper (l) oxide, Cu 2O(s), to copper(II) oxide, CuO(s), is an exothermic process, 

2Cu2O(s) + O2(g) → 4CuO(s)                    ΔH°rxn = -292.0 kJ/mol 

Calculate the energy released as heat (kJ) when 50.05 g of Cu 2O(s) undergo oxidation at constant pressure.


Solution

We’re being asked to determine the heat (q) released by the reaction of 50.05 g Cu2O


The given reaction is:

2 Cu2O(s) + O2(g)  4 CuO(s); ΔH˚rxn = –292.0 kJ/mol


From the balanced equation, we can see that the given ΔH˚rxn (–292.0 kJ) corresponds to 2 moles of Cu2O


Recall that at constant pressure, heat is equivalent to enthalpy.



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