If the chemical composition of the sample is known, then the answer is yes. However, equal masses of platinum and magnesium, for example, contain quite different numbers of atoms, because the Atomic Mass of platinum is much higher than that of magnesium.
The number of atoms is 1,50553521.10e23.
The total number of atoms contained in a 1,00 mole sample of helium is 6,022 140 857.10e23.
Take the actual sample weight of 13grams, and divide it by the atomic weight of chromium. This gives you your molar percentage of atoms. Now multiply this molar percentage by Avogadro's constant, the number of atoms in one mole, and this will give you your number of atoms in the sample.
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.
To calculate the evaporation rate, we need to know the number of atoms in the sample. The number of atoms in a 2 ml sample of liquid mercury can be calculated using Avogadro's number (6.022 x 10^23 atoms/mol for mercury). Then, divide the total number of atoms by the total number of seconds in 25 years to get the evaporation rate in atoms per second.
Which sample contains the greatest number of atoms. A sample of Mn that contains 3.29E+24 atoms or a 5.18 mole sample of I?The sample of _____ contains the greatest number of atoms.Answer:In order to compare the two samples, it is necessary to express both quantities in the same units. Since the question was phrased in terms of atoms, it is convenient to convert moles of I to atoms of I.The conversion factor between atoms and moles is Avogadro's number: 6.02 x 1023 "things" / molTo convert 5.18 moles of I to atoms of I:atoms I= 5.18 mol I6.02 x 1023 atoms I = 3.12E+24 atoms I1 mol IMultiply by atoms per mole. Moles cancel out.The sample of Mn contains 3.29E+24 atoms.Since 3.12E+24 is smaller than 3.29E+24, the sample of Mn contains the greatest number of atoms.
The number of atoms is 1,50553521.10e23.
The total number of atoms contained in a 1,00 mole sample of helium is 6,022 140 857.10e23.
All atoms have atomic numbers which are the same and the atoms have the same number of electrons.
Which sample contains the greatest number of atoms. A sample of Al that contains 8.18E+23 atoms or a 5.16 mole sample of S?The sample of______ contains the greatest number of atoms.Answer:In order to compare the two samples, it is necessary to express both quantities in the same units. Since the question was phrased in terms of atoms, it is convenient to convert moles of S to atoms of S.The conversion factor between atoms and moles is Avogadro's number: 6.02 x 1023 "things" / molTo convert 5.16 moles of S to atoms of S:atoms S=5.16 mol S6.02 x 1023 atoms S= 3.11E+24 atoms S1 mol SMultiply by atoms per mole. Moles cancel out.The sample of Al contains 8.18E+23 atoms.Since 3.11E+24 is larger than 8.18E+23, the sample of S contains the greatest number of atoms.
Take the actual sample weight of 13grams, and divide it by the atomic weight of chromium. This gives you your molar percentage of atoms. Now multiply this molar percentage by Avogadro's constant, the number of atoms in one mole, and this will give you your number of atoms in the sample.
Both samples contain the same number of carbon atoms because the number of atoms in a sample is determined by Avogadro's number (6.022 x 10^23) and not by the mass of the sample itself.
To find the percentage of copper-63 atoms in the sample, first add the number of copper-63 and copper-65 atoms together (1.76E4 + 7.88E3). Then, divide the number of copper-63 atoms by the total number of atoms and multiply by 100 to get the percentage. In this case, the percentage of copper-63 atoms in the sample is approximately 69.0%.
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.
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.
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.
To find the number of potassium atoms in a sample of K2Cr2O7, you first need to calculate the number of moles of K2Cr2O7 using its molar mass. Then, you can determine the number of moles of potassium atoms since there are 2 potassium atoms in each molecule of K2Cr2O7. Finally, use Avogadro's number (6.022 x 10^23) to convert the number of moles of potassium atoms to the actual number of atoms.