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: Consider the following reaction:4 NH3 (g) + 5 O2 (g) → 4 NO (g) + 6 H2O (g)If a container were to have 10 molecules of O 2 and 10 molecules of NH 3 initially, how many total molecules (reactants plus

Solution: Consider the following reaction:4 NH3 (g) + 5 O2 (g) → 4 NO (g) + 6 H2O (g)If a container were to have 10 molecules of O 2 and 10 molecules of NH 3 initially, how many total molecules (reactants plus

Problem

Consider the following reaction:

4 NH3 (g) + 5 O2 (g) → 4 NO (g) + 6 H2O (g)

If a container were to have 10 molecules of O 2 and 10 molecules of NH 3 initially, how many total molecules (reactants plus products) would be present in the container after this reaction goes to completion?

Solution

From the balance reaction equation, we can do a molecule to molecule comparison to determine how many molecules of products are formed. The limiting reactant would be the reactant that produces smaller number of products.

Balanced reaction: 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g)

We will use NO to determine the limiting reactant:

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