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: Calculate how many moles of NO2 form when each quantity of reactant completely reacts.2N2O5(g) → 4NO2(g) + O2(g)2.6 mol N2O5

Solution: Calculate how many moles of NO2 form when each quantity of reactant completely reacts.2N2O5(g) → 4NO2(g) + O2(g)2.6 mol N2O5

Problem

Calculate how many moles of NO2 form when each quantity of reactant completely reacts.
2N2O5(g) → 4NO2(g) + O2(g)

2.6 mol N2O5

Solution

2N2O5(g) → 4NO2(g) + O2(g)

Given the reaction above, we are asked to calculate the amount of NO2 produced from 2.6 mol N2O5.

First, we need to make sure that the reaction is balanced. We need to make sure that we have the same number of atoms for each element on each side


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