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: Ammonia (NH3) is prepared commercially by the reaction:  N2   +   3 H 2   →   2 NH 3  If 4.00 moles of N 2 and 8.0 moles of H 2 are mixed together and allowed to react, what is the limiting reagent

Problem

Ammonia (NH3) is prepared commercially by the reaction: 

N2   +   3 H 2   →   2 NH 3 

If 4.00 moles of N 2 and 8.0 moles of H 2 are mixed together and allowed to react, what is the limiting reagent and how many moles of the other reactant will remain after all of the limiting reagent has reacted?

 

A. N2 is the limiting reagent and 0.67 moles of H 2 will remain

B. H2 is the limiting reagent and 1.0 moles of N 2 will remain

C. N2 is the limiting reagent and 6.0 moles of H 2 will remain

D. H2 is the limiting reagent and 1.33 moles of N 2 will remain

E. H2 is the limiting reagent and 0.67 moles of N 2 will remain