Calculate the mass, in grams, of each sample. a. 1.1×10 23 gold atoms b. 2.82×10 22 helium atoms

Hey everyone. Our question here is asking us, how much do 6.2 times 10 to the 21st atoms of tungsten weight in g. To answer this question we're first going to meet to look at our periodic table and get the molar mass of tungsten. Now looking at our periodic table, we see that we have 183 0.84 g of tungsten per one mole of tungsten. So using that into our question, We're first going to take our 6.2 times 10 to the 21st atoms of tungsten and we're going to use avocados number to convert from Adams into moles. So we know that we have 6.02, 2 times 10 to the 23rd Adams of Tungsten per one mole of Tungsten plugging in our molar mass, We found that we have 183.84 g of tungsten per one mole of Tungsten. Now, when we calculate this out and cancel out our units, we end up with a value of 1. grams of truxton. 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.2 - Atoms & Elements

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Tro 4th Edition

Ch.2 - Atoms & Elements

Problem 89a,b

Chapter 2, Problem 89a,b

Calculate the mass, in grams, of each sample. a. 1.1×10²³ gold atoms b. 2.82×10²² helium atoms

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Identify the given quantity: 1.1 \times 10^{23} gold atoms.

Recall Avogadro's number, which is 6.022 \times 10^{23} atoms/mol. This number represents the number of atoms in one mole of a substance.

Determine the molar mass of gold (Au) from the periodic table, which is approximately 197 g/mol.

Calculate the number of moles of gold atoms by dividing the given number of atoms by Avogadro's number: \( \text{moles of Au} = \frac{1.1 \times 10^{23}}{6.022 \times 10^{23}} \).

Calculate the mass of the gold sample by multiplying the number of moles by the molar mass of gold: \( \text{mass of Au} = \text{moles of Au} \times 197 \text{ g/mol} \).

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Key Concepts

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

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). For gold (Au), the molar mass is approximately 197 g/mol. This value is essential for converting between the number of atoms and the mass of the substance, as it allows us to relate the atomic scale to macroscopic quantities.

Avogadro's Number

Avogadro's number, approximately 6.022 x 10^23, is the number of atoms, ions, or molecules in one mole of a substance. This constant is crucial for converting between the number of individual particles and the amount of substance in moles, enabling calculations involving atomic quantities and their corresponding masses.

Mass Calculation

To calculate the mass of a sample based on the number of atoms, one must first convert the number of atoms to moles using Avogadro's number. Then, by multiplying the number of moles by the molar mass of the substance, the total mass in grams can be determined. This process is fundamental in stoichiometry and quantitative chemistry.