Consider the following gas samples: 4.0 g of hydrogen gas, 4.0 g of helium gas, 1.0 mole of fluo

Consider the following gas samples: 4.0 g of hydrogen gas,...

Consider the following gas samples: $4.0 \mathrm{g}$ of hydrogen gas, 4.0 g of helium gas, 1.0 mole of fluorine gas, $44.0 \mathrm{g}$ of carbon dioxide gas, and 146 g of sulfur hexafluoride gas. Arrange the gas samples in order of increasing number of total atoms present.

Key Concepts

Moles and Molar Mass

This concept involves converting a given mass of a substance into moles by using the molar mass. The molar mass is the mass of one mole of a substance, which is calculated by adding up the atomic masses of all atoms in the molecule. Understanding how to calculate moles from a specified mass is fundamental when comparing amounts of substances, especially in gas samples.

Avogadro’s Number

Avogadro’s number, 6.022 x 10^23, is the number of particles in one mole of a substance. This concept bridges the macroscopic measurements (such as grams or moles) with the microscopic scale (number of molecules or atoms), allowing one to determine the total number of atoms or molecules present in a sample.

Molecular Formulas and Atomicity

This concept refers to analyzing the composition of a compound by examining its molecular formula, which indicates both the type and number of atoms present in a molecule. The term atomicity describes the number of atoms in a single molecule, and it is crucial when calculating the total number of atoms in a sample by multiplying the number of molecules (obtained from moles) by the number of atoms per molecule.

Transcript

00:01 Okay, so for this question, they want us to rank the following gas samples from increase in the order of increasing total number of atoms present.

00:12 All right, so the first thing that we should do is we should calculate how many atoms are present in all of the following gas samples.

00:19 And then we can put them in order.

00:22 So we have four grams of hydrogen gas, right? one mole of hydrogen gas is 2 grams and 1 mole is equal to 6 .023 times 10 to the 23rd atoms.

00:48 But we got to pay attention to h2.

00:51 So in 1 mole of h2 there are 2 atoms of a hydrogen.

00:57 So we have to multiply this by 2.

01:00 And we should get 2 .4092 times 10 to the 24 mows no 24 atoms now if they're asking like in this question they're asking for the total number of atoms present that's why we multiplied it by two but if they were only asking for the total number of hydrogen gas like h2 atoms present then we would we don't need to multiply it by two now for the second part it's four grams of helium one mole of helium one mole of helium is equal to 4 grams and we have 1 mole is equal to 6 .0 2 3 times 10 to the 23rd atoms right helium is only one one mole of helium only has one helium atom so we don't need to multiply by anything and we get 6 .023 times 10 to the 23rd now for the next one we have one mole of thorine gas so it's already in moles so we we don't need to convert into moles.

02:17 All we need is the conversion to atoms.

02:24 Now when we look at one mole of fluorine gas, it's f2, so there is, and one mole of fluorine gas are two fluorine atoms, so we have to multiply this by two.

02:34 We have 1 .2046 times 10 to the 24.

02:40 And now when we look at the next one, we have 44 grams of co2...

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