Ch.3 - Chemical ReactionsWorksheetSee 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: Nitrogen and hydrogen combine at high temperature, in the presence of a catalyst, to produce ammonia.N2 (g) + 3H2 (g) → 2NH3 (g) Assume 0.250 mol of N2 and 0.805 mol of H2 are present initially. After complete reaction, how many moles of ammonia are produced? How many moles of H2 remain? How many moles of N2 remain? What is the limiting reactant?

Problem

Nitrogen and hydrogen combine at high temperature, in the presence of a catalyst, to produce ammonia.

N2 (g) + 3H2 (g) → 2NH3 (g) 

Assume 0.250 mol of N2 and 0.805 mol of H2 are present initially. 

After complete reaction, how many moles of ammonia are produced? 

How many moles of H2 remain? 

How many moles of N2 remain? 

What is the limiting reactant?