Write 'true' or 'false' for each statement. (b) If the reaction 2 O 3 (g) → 3 O 2 (g) goes to completion and all O 3 is converted to O 2 , then the mass of O 3 at the beginning of the reaction must be the same as the mass of O 2 at the end of the reaction.

Hey everyone in this example, we need to consider the following reaction where all of our chlorine gas atoms were converted to chlorine gas molecules were told that the mass of our chlorine gas molecules produced is twice the mass of our chlorine gas atoms reacted. We need to consider whether the statement is true or false. So what we want to recall is our law of conservation of mass. And within this law we should recall that the mass of components in the reaction, she'll be conserved, not changed. And the second part of our law we should remember is that the mass of the reactant is going to equal the mass of our products. But according to our prompt, our mass of our product, which is our chlorine gas molecule is going to be twice the mass of our chlorine atoms that are reacted. So this is essentially negating our second law or second principle in our law of conservation of mass. And so we would say that therefore the statement is false because the mass of react ints In this case our reactant cl two gas must be equal to the mass. I'm sorry. This should say the mass of our reactant Cl gas must be equal to the mass of our cl two molecule. And so this is our final answer. To complete this example. I hope that everything I went through is clear. But if you have any questions, please leave them down below. Otherwise I will see everyone in the next practice video

Ch.3 - Chemical Reactions and Reaction Stoichiometry

All textbooks

Brown 14th Edition

Ch.3 - Chemical Reactions and Reaction Stoichiometry

Problem 9b

Chapter 3, Problem 9b

Write 'true' or 'false' for each statement. (b) If the reaction 2 O₃(g) → 3 O₂(g) goes to completion and all O₃ is converted to O₂, then the mass of O₃ at the beginning of the reaction must be the same as the mass of O₂ at the end of the reaction.

Verified step by step guidance

Identify the chemical reaction given: 2 O3(g) → 3 O2(g). This reaction describes the decomposition of ozone (O3) into oxygen (O2).

Understand the law of conservation of mass, which states that mass is neither created nor destroyed in a chemical reaction. Therefore, the total mass of reactants must equal the total mass of products.

Calculate the molar mass of O3 and O2. Ozone (O3) has a molar mass of 48 g/mol (16 g/mol per oxygen atom times 3), and oxygen (O2) has a molar mass of 32 g/mol (16 g/mol per oxygen atom times 2).

Set up a ratio based on the balanced chemical equation. For every 2 moles of O3 that react, 3 moles of O2 are produced. Use the molar masses to convert these mole ratios into mass ratios.

Apply the law of conservation of mass to confirm that the total mass of O3 used in the reaction equals the total mass of O2 produced, based on the calculated mass ratios and the stoichiometry of the reaction.

Verified Solution

Video duration:

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

Was this helpful?

Key Concepts

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

Law of Conservation of Mass

The Law of Conservation of Mass states that mass cannot be created or destroyed in a chemical reaction. This principle implies that the total mass of reactants must equal the total mass of products. In the context of the given reaction, if all O3 is converted to O2, the mass of O3 at the start must equal the mass of O2 produced at the end.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on balanced equations. It allows chemists to predict the quantities of substances consumed and produced. In the reaction 2 O3(g) → 3 O2(g), stoichiometry helps determine the relationship between the amounts of O3 and O2, reinforcing the conservation of mass.

Chemical Reaction Completion

A chemical reaction is said to go to completion when all reactants are converted into products. In this case, the complete conversion of O3 to O2 indicates that no O3 remains, and all its mass is transformed into O2. Understanding this concept is crucial for applying the Law of Conservation of Mass to the reaction in question.

Recommended video:

Guided course

00:47

Complete Ionic Equations

Related Practice

Textbook Question

Nitrogen monoxide and oxygen react to form nitrogen dioxide. Consider the mixture of NO and O2 shown in the accompanying diagram. The blue spheres represent N, and the red ones represent O. (a) How many molecules of NO2 can be formed, assuming the reaction goes to completion?

1381

views

Textbook Question

Nitrogen monoxide and oxygen react to form nitrogen dioxide. Consider the mixture of NO and O2 shown in the accompanying diagram. The blue spheres represent N, and the red ones represent O. (c) If the actual yield of the reaction was 75% instead of 100%, how many molecules of each kind would be present after the reaction was over?

1043

views

Textbook Question

Write 'true' or 'false' for each statement. (a) We balance chemical equations as we do because energy must be conserved.

1137

views

Textbook Question

A key step in balancing chemical equations is correctly identifying the formulas of the reactants and products. For example, consider the reaction between calcium oxide, CaO(s), and H2O1l2 to form aqueous calcium hydroxide. (b) Is it possible to balance the equation if you incorrectly identify the product as CaOH1aq2, and if so, what is the equation?

1125

views

Textbook Question

Balance the following equations: (c) Al(OH)₃(s) + H₂SO₄(l) → Al₂(SO₄)₃(s) + H₂O(l)

725

views

Textbook Question

Balance the following equations:

(a) HClO₄(aq) + P₄O₁₀(s) → HPO₃(aq) + Cl₂O₇(l)

(b) Au₂S₃(s + H₂(g) → Au(s) + H₂S(g)

667

views