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The molar mass of copper is approximately 63.5 g. To find how many of these are in our sample we must divide.0.0159/63.5 = 2.5 x 10 ^ -4 = 0.00025 moles.
Each mole contains the Avogadro number of atoms, i.e. 6.023 x 10 ^ 23, so in total we have
0.00025x 6.023 x 10 ^ 23 = 1.51 x 10 ^ 20 atoms approximately.
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The actual mass of an atom of argon is is 6.63x10-24g How many atoms are in a 40.0-g sample of argon?
To find the number of argon atoms in a 40.0-g sample, you first need to calculate the number of moles of argon in the sample using the molar mass of argon (39.95 g/mol). Then, you can use Avogadro's number (6.022x10^23 atoms/mol) to determine the number of atoms in that many moles of argon.
If a sample of pure sodium has a mass of 8.2 grams and sodium has an average atomic mass of 22.99 gmol how many sodium atoms are there in the sample?
To calculate the number of sodium atoms in the sample, first find the number of moles in the sample by dividing the mass (8.2 g) by the molar mass of sodium (22.99 g/mol). Then, use Avogadro's number (6.022 x 10^23 atoms/mol) to convert moles to atoms. Therefore, there are approximately 2.71 x 10^23 sodium atoms in a sample weighing 8.2 grams.
How many moles and how many atoms of zinc are in a sample weighing 34.9 g?
To find the number of moles of zinc, divide the sample's weight by the atomic weight of zinc (65.38 g/mol). This gives approximately 0.534 moles of zinc. To find the number of atoms, multiply the number of moles by Avogadro's number (6.022 x 10^23 atoms/mol) to get around 3.21 x 10^23 atoms in the sample.
How many moles of tantalum atoms are in a sample weighing 90.45 g?
To determine the number of moles, you need to divide the weight of the sample by the molar mass of tantalum. The molar mass of tantalum is approximately 180.95 g/mol. Therefore, 90.45 g / 180.95 g/mol = 0.500 moles of tantalum atoms.
A sample of gold has a mass of 5.00 x 10-3g. what amount of gold in atoms does the sample contain?
To determine the number of gold atoms in the sample, you can use the molar mass of gold (197 g/mol) to first find moles, then convert moles to atoms using Avogadro's number (6.022 x 10^23 atoms/mol). First, find moles: 5.00 x 10^-3 g ÷ 197 g/mol = 2.54 x 10^-5 mol. Then, convert moles to atoms: 2.54 x 10^-5 mol x 6.022 x 10^23 atoms/mol = 1.53 x 10^19 atoms.
How many atoms are present in a 15 mol sample of uranium?
Approx. 9.1024 atoms.
The mass of argon is 6.63 x 10-24g How many atoms are there in a 40.0 g sample argon?
First, calculate the number of moles in the 40.0 g sample of argon: 40.0 g / 39.948 g/mol = 1.00 mol. Then, use Avogadro's constant (6.022 x 10^23 atoms/mol) to find the number of atoms in 1.00 mol of argon, which is 6.022 x 10^23 atoms.
The mass of a sample of nickelaverage atomic mass 58.69 amu is 11.74g how many atoms does it contain?
To find the number of atoms in the sample, we need to first calculate the number of moles of nickel present in the sample using its molar mass. The molar mass of nickel is 58.69 g/mol. Dividing the mass of the sample by the molar mass gives us 0.200 moles of nickel. Finally, multiplying this by Avogadro's number (6.022 x 10^23 atoms/mol) gives us approximately 1.20 x 10^23 atoms in the sample.
How many atoms of phosphorus are in a 0.577 g sample?
1.12 x 10^22 atoms PFirst determine the number of moles in the 0.577 g sample of phosphorus, determine the number of moles in the sample. Then multiply the moles by 6.022x10^23 atoms/mol.0.577 g P x (1 mol P/30.974 g P) x (6.022x10^23 atoms P/1 mol P) = 1.12 x 10^22 atoms P
How many atoms are there in a 0.250 mol sample of vanadium?
0.250 X Avogadro's Number = 1.51 X 1023, to the justified number of significant digits.
How many moles of P are there in a sample of P that contains 3.78E plus 24 atoms?
The conversion factor between atoms and moles is Avogadro's number: 6.02 x 1023 "things" / molTo convert atoms to moles:moles P= 3.78E+24 atoms P1 mol P = 6.28 mol P6.02 x 1023 atoms PMultiply by moles per atom. Atoms cancel out.
The actual mass of an atom of argon is is 6.63x10-24g How many atoms are in a 40.0-g sample of argon?
To find the number of argon atoms in a 40.0-g sample, you first need to calculate the number of moles of argon in the sample using the molar mass of argon (39.95 g/mol). Then, you can use Avogadro's number (6.022x10^23 atoms/mol) to determine the number of atoms in that many moles of argon.
If a sample of pure sodium has a mass of 8.2 grams and sodium has an average atomic mass of 22.99 gmol how many sodium atoms are there in the sample?
To calculate the number of sodium atoms in the sample, first find the number of moles in the sample by dividing the mass (8.2 g) by the molar mass of sodium (22.99 g/mol). Then, use Avogadro's number (6.022 x 10^23 atoms/mol) to convert moles to atoms. Therefore, there are approximately 2.71 x 10^23 sodium atoms in a sample weighing 8.2 grams.
How many moles and how many atoms of zinc are in a sample weighing 34.9 g?
To find the number of moles of zinc, divide the sample's weight by the atomic weight of zinc (65.38 g/mol). This gives approximately 0.534 moles of zinc. To find the number of atoms, multiply the number of moles by Avogadro's number (6.022 x 10^23 atoms/mol) to get around 3.21 x 10^23 atoms in the sample.
How many atoms of sodium na are in 7 mol of sodium answer in units of atoms?
the constant Mole (mol): 6.02 x 10^23 are how many atoms you have per mol so the answer can be 7 mol atoms or 6.02 x 10^23 atoms per mol x 7 actual answer is 4.214 X10^24 atoms in 7 mol
How many moles of tantalum atoms are in a sample weighing 90.45 g?
To determine the number of moles, you need to divide the weight of the sample by the molar mass of tantalum. The molar mass of tantalum is approximately 180.95 g/mol. Therefore, 90.45 g / 180.95 g/mol = 0.500 moles of tantalum atoms.
A sample of gold has a mass of 5.00 x 10-3g. what amount of gold in atoms does the sample contain?
To determine the number of gold atoms in the sample, you can use the molar mass of gold (197 g/mol) to first find moles, then convert moles to atoms using Avogadro's number (6.022 x 10^23 atoms/mol). First, find moles: 5.00 x 10^-3 g ÷ 197 g/mol = 2.54 x 10^-5 mol. Then, convert moles to atoms: 2.54 x 10^-5 mol x 6.022 x 10^23 atoms/mol = 1.53 x 10^19 atoms.
