Balance the equation and calculate how many moles of O 2 form when each quantity of reactant completely reacts. N 2 O 5 ( g) → NO 2 (g) + O 2 (g) a. 1.2 mol N 2 O 5

Hey everyone. Our question here asked if 5.7 moles of di nitrogen Penta oxide react, how many moles of nitrogen dioxide form, Looking at our reaction, we can see that this is unbalanced. So let's go ahead and balance this out first before answering our question. So in our react inside we have two of nitrogen and five of oxygen and in our product side we have one of nitrogen And four of oxygen. Now, in order to balance this out, we're going to need to change our oxygen in our reacting side to be an even number. So we can do this by multiplying our react inside by two. Now this will change our nitrogen into four And our oxygen's into 10. Since we did this, we're going to have to balance out our product side as well. So by multiplying nitrogen dioxide by four, We end up with four of nitrogen and a total of 10 oxygen's which gives us our balanced chemical equation. Now we can go ahead and move on with our question. Starting off with 5.7 mol of di nitrogen Penta oxide, we can see that in our balance chemical reaction We have two moles of di nitrogen Penta oxide and this is equivalent to formals of nitrogen dioxide. Now, when we calculate this out, We end up with a total of 22.8 mole of nitrogen dioxide, Which we can round up to 23 and this is going to be our final answer. So I hope this made sense and let us know if you have any questions

Ch.4 - Chemical Reactions and Chemical Quantities

All textbooks

Tro 6th Edition

Ch.4 - Chemical Reactions and Chemical Quantities

Problem 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

Verified step by step guidance

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.>

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Video duration:

Was this helpful?

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.

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.

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.

Recommended video:

Guided course

01:25

Mole Concept

Related Practice

Textbook Question

Write the balanced chemical equation for the reaction of aqueous potassium hydroxide with aqueous iron(III) chloride to form solid iron(III) hydroxide and aqueous potassium chloride.

Textbook Question

Balance each chemical equation. b. Co(NO₃)₃(aq) + (NH₄)₂S(aq) → Co₂S₃(s) + NH₄NO₃(aq)

views

Textbook Question

Consider the unbalanced equation for the neutralization of acetic acid: HC₂H₃O₂(aq) + Ba(OH)₂(aq) → H₂O(l) + Ba(C₂H₃O₂)₂(aq) Balance the equation and determine how many moles of Ba(OH)₂ are required to completely neutralize 1.22 mol of HC₂H₃O₂.

Textbook Question

Balance the equation and calculate how many moles of N₂ form when each quantity of reactant completely reacts. N₂H₄(l) → NH₃(g) + N₂(g) c. 33.9 g N₂H₄

Textbook Question

Consider the balanced equation:

SiO₂(s) + 3 C(s) → SiC(s) + 2 CO(g)

Complete the table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, as well as the moles of each product that forms. If the number of moles of a product is provided, fill in the required amount of each reactant to make that amount of product, as well as the amount of the other product that forms.

Textbook Question

Consider the balanced equation:

SiO₂(s) + 3 C(s) → SiC(s) + 2 CO(g)

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

Verified video answer for a similar problem:

Key Concepts

Balancing Chemical Equations

Stoichiometry

Mole Concept

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