which sample contians the greatest number of atoms. a)10.0g He b)25.0g Ne c)115g Xe

Convert each to moles. moles = grams/molar mass. The one containing the largest number of moles will contain the largest number of atoms.

Oh, I love a good atom party! Let's see which sample contains the most atoms. We'll use Avogadro's number here, which tells us that one mole of any substance contains 6.02 x 10^23 atoms. So, let's do some math with our hilarious hats on!

a) 10.0g He: First, we need to find the number of moles of He in this sample. The molar mass of helium (He) is about 4 g/mol. So, by dividing 10 g by 4 g/mol, we get 2.5 moles of He. And since we know that one mole contains 6.02 x 10^23 atoms, we can multiply 2.5 moles by 6.02 x 10^23 atoms/mole to get approximately 1.505 x 10^24 atoms of He.

b) 25.0g Ne: Similarly, let's find the number of moles of Ne in this sample. The molar mass of neon (Ne) is about 20 g/mol. So, by dividing 25 g by 20 g/mol, we get 1.25 moles of Ne. And by multiplying 1.25 moles by 6.02 x 10^23 atoms/mole, we end up with roughly 7.525 x 10^23 atoms of Ne.

c) 115g Xe: Last but not least, we'll determine the number of moles of Xe in this sample. The molar mass of xenon (Xe) is about 131 g/mol. So, dividing 115 g by 131 g/mol gives us approximately 0.877 moles of Xe. And multiplying 0.877 moles by 6.02 x 10^23 atoms/mole, we find ourselves with about 5.284 x 10^23 atoms of Xe.

Drumroll, please! The grand winner, with the greatest number of atoms, is... (cue silly drum sounds) option a) 10.0g He! With approximately 1.505 x 10^24 atoms, helium takes the atom crown in this atom-packed competition. But hey, all atoms are unique and special, just like you!

To determine which sample contains the greatest number of atoms, we can convert each sample's mass to the number of moles using the atomic mass of the elements and Avogadro's number.

a) 10.0g He:
The atomic mass of helium (He) is approximately 4 grams/mole.
To convert grams to moles, we divide the mass by the atomic mass:
10.0 g He / 4.0 g/mol He = 2.5 mol He

b) 25.0g Ne:
The atomic mass of neon (Ne) is approximately 20 grams/mole.
To convert grams to moles:
25.0 g Ne / 20.0 g/mol Ne = 1.25 mol Ne

c) 115g Xe:
The atomic mass of xenon (Xe) is approximately 131 grams/mole.
To convert grams to moles:
115 g Xe / 131g/mol Xe = 0.878 mol Xe

Comparing the number of moles, we can see that 10.0g He has the largest number of moles, and therefore, the greatest number of atoms.

To determine which sample contains the greatest number of atoms, we need to compare the number of atoms present in each sample using their respective atomic masses.

To calculate the number of atoms in a given sample, we can use the relationship between mass, moles, and Avogadro's number (6.02 x 10^23). The formula is as follows:

Number of atoms = (mass of sample in grams) / (molar mass) * Avogadro's number

Let's calculate the number of atoms for each sample:

a) 10.0g He:
The molar mass of helium (He) is approximately 4.00 g/mol.
Number of atoms = (10.0g He) / (4.00 g/mol) * (6.02 x 10^23) = 1.505 x 10^24 atoms

b) 25.0g Ne:
The molar mass of neon (Ne) is approximately 20.18 g/mol.
Number of atoms = (25.0g Ne) / (20.18 g/mol) * (6.02 x 10^23) = 1.491 x 10^24 atoms

c) 115g Xe:
The molar mass of xenon (Xe) is approximately 131.29 g/mol.
Number of atoms = (115g Xe) / (131.29 g/mol) * (6.02 x 10^23) = 6.02 x 10^24 atoms

Therefore, the sample that contains the greatest number of atoms is c) 115g Xe, with 6.02 x 10^24 atoms.