Ch.6 - Thermochemistry WorksheetSee all chapters
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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: For the reactionH2(g) + 1/2O2(g) --> H2O(l)              deltaH = –286 kJ/molcalculate the enthalpy change when 2.66 g of water is produced.1. 761 kJ2. –42.2 kJ3. –761 kJ4. 108 kJ5. 42.2 kJ

Problem

For the reaction

H2(g) + 1/2O2(g) --> H2O(l)              deltaH = –286 kJ/mol

calculate the enthalpy change when 2.66 g of water is produced.

1. 761 kJ

2. –42.2 kJ

3. –761 kJ

4. 108 kJ

5. 42.2 kJ

Solution

We’re being asked to determine the enthalpy change when 2.66 g H2O is produced

The given reaction is:

2(g) + 1/2 O2(g) H2O(g); ΔH = –286 kJ/mol


From the balanced equation, we can see that the given ΔH˚rxn (-286 kJ/mol) corresponds to 1 mole of H2O


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