(a) What are the mole fractions of H 2 in a mixture of 15.08 g of O 2 , 8.17 g of N 2 , and 2.64 g of H 2 ?

Hey there, welcome back. So we have a vessel that contains carbon monoxide, hydrogen gas and oxygen gas. So, we have a mole fractions given to us of hydrogen gas and oxygen gas. There are points 17 and 170.62 respectively. We want the mole fraction of the other gas of carbon monoxide. So we want um mole fraction of C. O. Which is going to equal to moles of C. O. Over the total number of moles. Now we don't have the total number of moles. We don't have walls of SEO, but we do have the mole fractions of the other gasses. So, mole fraction of H two is equal to 20.17. So what does this actually mean? Well, it means that there are . moles for every one mole of the mixture of the gasses. Right? And the same thing for 02. So mole fraction of 02 Equals 2.62. That just means that there are .62 moles for every one mole of this mixture of gasses. So, we're not saying that there is exactly one mole um total of this mixture. What we can just assume that we do have one mole, we can treat that as one mole total and plug that into here and then find moles of C. O. Because moles of C. O. Is going to equal to the total moles, which is, let's say one mole oops, One will subtract moles of H two and 02. So subtract points 17 moles And .62 moles. Right? That will give us smells of ceo relative To the mixture. So that would be .21 moles of C. O. So that means that the mole fraction of C. O. Here is just going to be 00. moles divided by the total moles one goal and that is just 10.21. Alright, so that is going to be the answer. So again, we're not necessarily saying that there are, there's only one mole of this mixture, but the mole fractions are giving us how many moles per one mole of the mixture and that will allow us to find the mole fraction of the other gas that is left over. Because here we knew, we knew H. Two and 02 and we can find Ceo because we had the rest of them. Alright folks, if you have any questions about the slaughter snow and we'll see you in the next video.

Ch.10 - Gases

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Brown 14th Edition

Ch.10 - Gases

Problem 72a3

Chapter 10, Problem 72a3

(a) What are the mole fractions of H₂ in a mixture of 15.08 g of O₂, 8.17 g of N₂, and 2.64 g of H₂?

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Step 1: The first step is to convert the mass of each component to moles. This is done by dividing the mass of each component by its molar mass. The molar mass of O2 is 32.00 g/mol, N2 is 28.01 g/mol, and H2 is 2.02 g/mol.

Step 2: After converting the mass of each component to moles, add up the total number of moles in the mixture. This is done by adding the number of moles of O2, N2, and H2 together.

Step 3: The mole fraction of a component in a mixture is the number of moles of that component divided by the total number of moles in the mixture. So, to find the mole fraction of H2, divide the number of moles of H2 by the total number of moles in the mixture.

Step 4: The result from step 3 is the mole fraction of H2 in the mixture. This value is a ratio and does not have units.

Step 5: Remember that the mole fraction is a way of expressing the concentration of a component in a mixture. It tells us what fraction of the total number of moles in the mixture is made up by a particular component.

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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 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 10²³) of entities, whether they are atoms, molecules, or ions. This concept is essential for converting grams of a substance to moles, which is necessary for calculating mole fractions.

Mole Fraction

Mole fraction is a way of expressing the concentration of a component in a mixture. It is defined as the ratio of the number of moles of a specific component to the total number of moles of all components in the mixture. Mole fractions are dimensionless and provide a useful means of comparing the relative amounts of different substances in a mixture.

Mass to Moles Conversion

To calculate mole fractions, it is necessary to convert the mass of each component in the mixture to moles. This is done using the formula: moles = mass (g) / molar mass (g/mol). Knowing the molar masses of O₂, N₂, and H₂ allows for the determination of the number of moles of each gas, which is crucial for finding the total moles and subsequently the mole fractions.

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Mass and Moles Conversion

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Textbook Question

At an underwater depth of 100 m, the pressure is 1.106 MPa. What should the partial pressure of oxygen be in the diving gas for the mole fraction of oxygen in the mixture to be 0.21, the same as in air?

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Textbook Question

(a) What are the mole fractions of O₂ in a mixture of 15.08 g of O₂, 8.17 g of N₂, and 2.64 g of H₂?

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Textbook Question

(a) What are the mole fractions of N₂ in a mixture of 15.08 g of O₂, 8.17 g of N₂, and 2.64 g of H₂?

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Textbook Question

(b) What is the partial pressure in atm of each component of this mixture if its held in a 15.50-L vessel at 15 °C?

Textbook Question

A quantity of N2 gas originally held at 531.96 kPa pressure in a 1.00-L container at 26 °C is transferred to a 12.5-L container at 20 °C. A quantity of O2 gas originally at 531.96 kPa and 26 °C in a 5.00-L container is transferred to this same container. What is the total pressure in the new container?

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Textbook Question

A sample of 3.00 g of SO₂(g) originally in a 5.00-L vessel at 21 °C is transferred to a 10.0-L vessel at 26 °C. A sample of 2.35 g of N₂(g) originally in a 2.50-L vessel at 20 °C is transferred to this same 10.0-L vessel. (a) What is the partial pressure of SO₂(g) in the larger container? (b) What is the partial pressure of N₂(g) in this vessel?

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(a) What are the mole fractions of H2 in a mixture of 15.08 g of O2, 8.17 g of N2, and 2.64 g of H2?

Verified video answer for a similar problem:

Key Concepts

Mole Concept

Mole Fraction

Mass to Moles Conversion

(a) What are the mole fractions of H₂ in a mixture of 15.08 g of O₂, 8.17 g of N₂, and 2.64 g of H₂?