Determine the number of moles of oxygen atoms in each sample. a. 4.88 mol H 2 O 2 b. 2.15 mol N 2 O c. 0.0237 mol H 2 CO 3 d. 24.1 mol CO 2

Hello, everyone. Today, we have the following problem, determine the number of moles of oxygen apps in each sample. So we will first start with a, we have 4.88 moles. So to find the number of moles of oxygen, you have to multiply by the multi mole ratio. So that means that if we have one more of our hydrogen peroxide, we look at the molecule itself and we see that we have two moles of oxygen within it. So we have two moles of oxygen. And so if we cross our units out and multiply these two numbers, we will receive 9.76 moles of oxygen as our answer. So we can eliminate choices A and D, we then look at our be and we see that we have our nitrous oxide. So once again, we have our one mole of that nitrous oxide. And we see in a molecule, we also have one mole of our oxygen, we then can cancel our units and arrive at an answer of 2.15 moles of oxygen for seat. Once he has the same situation, we have one more or carbonate. And in that carbon, we have three moles of our oxygen. So our units cancel. When our units cancel, we arrive in an answer of 0.0711 moles of oxygen. Eliminating any answer. Choice C is our answer. But let's do d we then have one mole of our carbon dioxide. And in that mole molecule, we have two moles of oxygen. And when we solve the math, we arrive at an answer of 48.2 moles of oxygen atoms. And so with that, we conclude, conclude that our answer is b overall, I hope this helped. And until next time.

Ch.3 - Molecules, Compounds & Chemical Equations

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Tro 4th Edition

Ch.3 - Molecules, Compounds & Chemical Equations

Problem 82

Chapter 3, Problem 82

Determine the number of moles of oxygen atoms in each sample. a. 4.88 mol H₂O₂ b. 2.15 mol N₂O c. 0.0237 mol H₂CO₃ d. 24.1 mol CO₂

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Identify the chemical formula of each compound to determine the number of oxygen atoms per molecule. For H2O2, there are 2 oxygen atoms; for N2O, there is 1 oxygen atom; for H2CO3, there are 3 oxygen atoms; and for CO2, there are 2 oxygen atoms.

Use the mole concept, which states that 1 mole of a substance contains Avogadro's number of entities (molecules, atoms, etc.). Here, focus on the number of moles of each compound given in the problem.

Multiply the number of moles of each compound by the number of oxygen atoms per molecule of that compound. This will give you the total number of moles of oxygen atoms in each sample.

For H2O2, multiply the moles of H2O2 by 2 to find the moles of oxygen atoms. For N2O, multiply the moles of N2O by 1. For H2CO3, multiply the moles of H2CO3 by 3. For CO2, multiply the moles of CO2 by 2.

Summarize the results for each compound to find the total moles of oxygen atoms in each sample.

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Key Concepts

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

Mole Concept

The mole is a fundamental unit in chemistry that quantifies the amount of substance. One mole contains approximately 6.022 x 10^23 entities, such as atoms or molecules. Understanding the mole concept is essential for converting between the number of moles and the number of particles, which is crucial for solving problems involving chemical reactions and stoichiometry.

Chemical Formula Interpretation

Chemical formulas represent the composition of compounds, indicating the types and numbers of atoms present. For example, H2O2 (hydrogen peroxide) contains two hydrogen atoms and two oxygen atoms. By interpreting these formulas, one can determine the number of moles of specific atoms in a given number of moles of the compound, which is necessary for the question at hand.

Stoichiometry

Stoichiometry is the area of chemistry that deals with the relationships between the quantities of reactants and products in chemical reactions. It allows chemists to calculate the amount of substances consumed and produced in a reaction based on balanced chemical equations. This concept is vital for determining the number of moles of oxygen atoms in various compounds as presented in the question.