Ch.14 - Chemical EquilibriumWorksheetSee 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: The first step in HNO3 production is the catalyzed oxidation of NH3. Without a catalyst, a different reaction predominates:         4NH 3(g) + 3O2(g) ⥫⥬ 2N2(g) + 6H2O(g)When 0.0150 mol of NH3(g) and 0

Problem

The first step in HNO3 production is the catalyzed oxidation of NH3. Without a catalyst, a different reaction predominates:
         4NH 3(g) + 3O2(g) ⥫⥬ 2N2(g) + 6H2O(g)
When 0.0150 mol of NH3(g) and 0.0150 mol of O2(g) are placed in a 1.00-L container at a certain temperature, the N2 concentration at equilibrium is 1.96×10−3 M. Calculate Kc.