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: A miniature volcano can be made in the laboratory with ammonium dichromate. When ignited, it decomposes in a fiery display. (NH4)2Cr2O7 (s) → N2 (g) + 4H2O (g) + Cr2O3 (s) If 0.76 g of ammonium dichromate is used, and the gases from this reaction are trapped in a 15.1 L flask at 29°C, what is the total pressure of the gas in the flask? What are the partial pressures of N2 and H2O? 

Problem

A miniature volcano can be made in the laboratory with ammonium dichromate. When ignited, it decomposes in a fiery display. 

(NH4)2Cr2O7 (s) → N(g) + 4H2O (g) + Cr2O3 (s) 

If 0.76 g of ammonium dichromate is used, and the gases from this reaction are trapped in a 15.1 L flask at 29°C, what is the total pressure of the gas in the flask? What are the partial pressures of N2 and H2O?