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: In some aquatic ecosystems, nitrate (NO3-) is converted to nitrite (NO2-), which then decomposes to nitrogen and water. As an example of this second reaction, consider the decomposition of ammonium nitrite: NH4NO2 (aq) → N2 (g) + 2H2 O (l) What would be the change in pressure in a sealed 10.0 L vessel due to the formation of N  2 gas when the ammonium nitrite in 2.40 L of 1.340 M NH4NO2 decomposes at 25 °C?

Problem

In some aquatic ecosystems, nitrate (NO3-) is converted to nitrite (NO2-), which then decomposes to nitrogen and water. As an example of this second reaction, consider the decomposition of ammonium nitrite: 

NH4NO2 (aq) → N2 (g) + 2H2 O (l) 

What would be the change in pressure in a sealed 10.0 L vessel due to the formation of N  2 gas when the ammonium nitrite in 2.40 L of 1.340 M NH4NO2 decomposes at 25 °C?