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How many atoms are in a gold ring that has a mass of 19.7 grams?
Wiki User
∙ 14y ago
Well, firstly you need to know if it is pure gold. Assuming that it is, convert the grams to moles
19.7g Au x 1molAu/197.0gAu = 0.1moles Au
And then, to get the number of atoms in 0.1 moles of gold, multiply it by Avogadro's number, 6.22x10^23 atoms per mole
0.1mol Au x 6.22x10^23atoms/mole = 6.22x10^22
Wiki User
∙ 14y ago
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How many atoms of gold are in 5 grams of gold?
Atomic mass of Ag: 107.9 grams5.00 grams × (6.02 × 1023 atoms) / (107.9 grams) = 2.79 × 1022 atoms Ag
What is the mass in grams of 2x1012 atoms of potassium?
What is the mass, in grams, of 2 × 1012 atoms of potassium?
Au contains how many gold atoms?
This depends on the mass of the gold sample.
What is the mass of 175 atoms of gold?
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How many atoms are present in 5 grams of AuCl3?
For this problem, the atomic mass is required. Take the mass in grams and divide it by the atomic mass. Then multiply it by Avogadro's constant, 6.02 × 1023. AuCl3= 303.5 grams5.00 grams AuCl3 / (303.5 grams) × (6.02 × 1023 atoms) = 9.92 × 1021 atoms
How many atoms of gold are in 5 grams of gold?
Atomic mass of Ag: 107.9 grams5.00 grams × (6.02 × 1023 atoms) / (107.9 grams) = 2.79 × 1022 atoms Ag
How many atoms does 100 grams of gold have?
Gold has a molar mass of 196.96655 grams per mole. 100 grams then is equal to .508 moles which makes 3.059 E23 atoms of gold.
5.6 moles of gold contain how many atoms?
5.0 grams gold (1 mole Au/197.0 grams)(6.022 X 1023/1 mole Au) = 1.5 X 1022 atoms of gold ===================
What is the mass in grams of 2x1012 atoms of potassium?
What is the mass, in grams, of 2 × 1012 atoms of potassium?
How many gold atoms does Au contain?
This depends on the mass of the gold sample.
Au contains how many gold atoms?
This depends on the mass of the gold sample.
What is the mass of 175 atoms of gold?
equation: g= 175 atoms x 1 mol/6.02x10^23 x 196.97g/1 mol ---> 175 atoms of gold weigh 5.73x10^-20 grams.
What is the mass of 5.0g of Fe how many atoms are present?
For this problem, the atomic mass is required. Take the mass in grams and divide it by the atomic mass. Then multiply it by Avogadro's constant, 6.02 × 1023.5.0 grams Fe / (55.9 grams) × (6.02 × 1023 atoms) = 5.38 × 1022 atoms
How many atoms of sulfur are in 3.86 g?
For this problem, the atomic mass is required. Take the mass in grams and divide it by the atomic mass. Then multiply it by Avogadro's constant, 6.02 × 1023.3.86 grams S / (32.1 grams) × (6.02 × 1023 atoms) = 7.24 × 1022 atoms
How many atoms in 1000 g of carbon?
For this problem, the atomic mass is required. Take the mass in grams and divide it by the atomic mass. Then multiply it by Avogadro's constant, 6.02 × 1023.1000 grams C / (12.0 grams) × (6.02 × 1023 atoms) = 5.02 × 1025 atoms
How many atoms are in 1.9 g Carbon?
Atomic mass of carbon: 12.0 grams1.90 grams × (6.02 × 1023 atoms) / (12.0 grams) = 9.53 × 1022 atoms C
How many atoms are present in 5 grams of AuCl3?
For this problem, the atomic mass is required. Take the mass in grams and divide it by the atomic mass. Then multiply it by Avogadro's constant, 6.02 × 1023. AuCl3= 303.5 grams5.00 grams AuCl3 / (303.5 grams) × (6.02 × 1023 atoms) = 9.92 × 1021 atoms
