Answer :
a scientist has a 98.3 g sample of silicon. The number of silicon atoms that are in this sample is: B. 2.11 x 1023 atoms
Given the following data: • Mass of silicon = 98.3 grams. Scientific data:• Avogadro's number = 6.02 x 1023• Molar mass of silicon = 28.09 g/mol.
To determine the number of silicon atoms that are in this sample: First of all, we would determine the number of moles contained in 98.3 grams of silicon. Number of moles =mass molar mass/ Number of moles = 98.3/28.09. Number of moles = 3.4995 moles. By stoichiometry: 1 mole of silicon = 6.02 × 1023 atoms, 3.4995 moles of silicon = X atoms. Cross-multiplying, we have: X = 6.02 × 1023 × 3.4995. X = 2.11 × 1023 atoms
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Final answer:
The 98.3 g sample of silicon contains approximately 2.1 x 10²⁴ atoms. This is calculated by first converting the weight to moles using the atomic mass of silicon, and then multiplying the resulting moles by Avogadro's number.
Explanation:
To find out how many atoms of silicon are in a 98.3 g sample, we need to use Avogadro's number and the atomic mass of silicon. Avogadro's number is a constant, defining the number of entities (atoms in this case) in one mole of a substance, which is 6.022 x 10²³. The atomic mass of silicon is approximately 28.1 g.
First, convert the mass of silicon to moles using the atomic mass, which gives us: 98.3 g / 28.1 g/mol ≈ 3.5 moles.
Then, multiply the number of moles by Avogadro's number to get the total number of atoms: 3.5 moles x 6.022 x 10²³ atoms/mol ≈ 2.1 x 10²⁴ atoms.
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