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 total volume of hydrogen gas needed to fill the Hinderburg was 2.00 x 108 L at 1.00 atm and 25.0°C. How much energy was evolved when it burned?Hint-Use the Ideal Gas Law to obtain the moles of hyd

Problem

The total volume of hydrogen gas needed to fill the Hinderburg was 2.00 x 108 L at 1.00 atm and 25.0°C. How much energy was evolved when it burned?

Hint-Use the Ideal Gas Law to obtain the moles of hydrogen gas. 

2H2 (g) + O2 (g) → 2H2O (l)      ΔH = -572 kJ

a. 2.86 x 104 kJ

b. 5.72 x 1010 kJ

c. 8.18 x 106 kJ

d. 35 x 1011 kJ 

e. 2.34 x 10kJ