Ch.9 - Bonding & Molecular StructureWorksheetSee 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

Bond Energy

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Sections
Chemical Bonds
Lattice Energy
Lattice Energy Application
Born Haber Cycle
Dipole Moment
Lewis Dot Structure
Octet Rule
Formal Charge
Resonance Structures
Additional Practice
Bond Energy
Additional Practice

Solution: 2 H2S(g) + 3 O2(g) --> 2 SO2(g) + 2 H2O(g)Calculate the ∆Hrxn in kJ.Average bond energies:H—S 347 kJ/molO = O 495 kJ/molO—H 463 kJ/mol

Solution: 2 H2S(g) + 3 O2(g) --> 2 SO2(g) + 2 H2O(g)Calculate the ∆Hrxn in kJ.Average bond energies:H—S 347 kJ/molO = O 495 kJ/molO—H 463 kJ/mol

Problem

2 H2S(g) + 3 O2(g) --> 2 SO2(g) + 2 H2O(g)

Calculate the ∆Hrxn in kJ.

Average bond energies:

H—S 347 kJ/mol

O = O 495 kJ/mol

O—H 463 kJ/mol



Solution

To calculate the ΔH°rxn using bond energies, we’re going to use the following equation:

Let’s first figure out what kind of bonds and how many moles are present in each reactants and products because the given bond energies are per mole.

Balanced Reaction:  2 H2S(g) + 3 O2(g) → 2 SO2(g) + 2 H2O(g)

*always make sure that the given reaction is balanced


Draw the structure of each compound.

Reactants:

• H2S:

View the complete written solution...
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