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: Predict whether the following reactions will be exothermic or endothermic.a. N2(g) + 3H2(g) → 2NH3(g)b. S(g) + O2(g) → SO2(g)c. 2H2O(g) → 2H2(g) + O2(g)d. 2F(g) → F2(g)


Predict whether the following reactions will be exothermic or endothermic.

a. N2(g) + 3H2(g) → 2NH3(g)

b. S(g) + O2(g) → SO2(g)

c. 2H2O(g) → 2H2(g) + O2(g)

d. 2F(g) → F2(g)


We’re being asked to classify each given reaction as exothermic or endothermic

Recall that:

Exothermic reactions: lose energy and involve bonds forming; ΔH is negative

Endothermic reactions: gain energy and involve bonds breaking; ΔH is positive

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