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Ch.4 - Chemical Reactions and Chemical Quantities
Tro - Chemistry: A Molecular Approach 6th Edition
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Not the one you use?Change textbook
All textbooksTro 6th EditionCh.4 - Chemical Reactions and Chemical QuantitiesProblem 33a
Chapter 4, Problem 33a

Balance the equation and calculate how many moles of O2 form when each quantity of reactant completely reacts. N2O5( g) → NO2(g) + O2(g) a. 1.2 mol N2O5

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N_2O_5(g) \(\rightarrow\) NO_2(g) + O_2(g)
Start by balancing the nitrogen atoms. Since there are 2 nitrogen atoms in N_2O_5, you need 2 NO_2 molecules on the product side: N_2O_5(g) \(\rightarrow\) 2 NO_2(g) + O_2(g).
There are 5 oxygen atoms in N_2O_5. On the product side, 2 NO_2 molecules contribute 4 oxygen atoms, so you need 1 more oxygen atom from O_2. Therefore, the balanced equation is: 2 N_2O_5(g) \(\rightarrow\) 4 NO_2(g) + O_2(g).
From the balanced equation, 2 moles of N_2O_5 produce 1 mole of O_2.
Use the mole ratio to find the moles of O_2 produced from 1.2 moles of N_2O_5.>

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Balancing Chemical Equations

Balancing chemical equations is essential to ensure that the number of atoms for each element is the same on both sides of the equation. This reflects the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction. In the given reaction, N2O5 decomposes into NO2 and O2, and balancing the equation will help determine the stoichiometric relationships between the reactants and products.
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Stoichiometry

Stoichiometry involves the calculation of reactants and products in chemical reactions based on balanced equations. It allows chemists to predict how much of a product will form from a given amount of reactant. In this case, once the equation is balanced, stoichiometric coefficients can be used to determine the moles of O2 produced from the moles of N2O5 that react.
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Mole Concept

The mole concept is a fundamental principle in chemistry that relates the mass of a substance to the number of particles it contains. One mole of any substance contains Avogadro's number (approximately 6.022 x 10^23) of entities, whether they are atoms, molecules, or ions. Understanding this concept is crucial for converting between moles and grams, and for calculating the amount of O2 produced in the reaction based on the initial moles of N2O5.
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