If you determined that the volume of a silver bar is 100 mL, how many atoms of silver would be in the bar? The density of silver is 10.5 g/mL.

10.5 g/mL * 100 mL = 1050 g of silver
1050 g silver * ( 1 mol silver/107.8682g) = 9.734 mol silver
9.734 moles silver * 6.022E23 atoms/ mole = 5.861E24 atoms of silver
Where molar mass if silver = 107.8682g/mol Avogadro's number = 6.022E23 atoms/moles

Answered by r0wieo7 | 2024-06-10

There are approximately 5.86 ∗ 1 0 24 a t o m s of silver in the 100 mL silver bar.
To determine the number of atoms in a silver bar, you can follow these steps:
Calculate the mass of the silver bar:
Mass (g) = Volume (mL) x Density (g/mL)
Mass = 100 mL x 10.5 g/mL = 1050 g
Calculate the molar mass of silver (Ag):
The molar mass of silver (Ag) is approximately 107.87 g/mol.
Calculate the number of moles of silver in the bar:
Moles = Mass (g) / Molar Mass (g/mol)
Moles = 1050 g / 107.87 g/mol ≈ 9.73 moles
Calculate Avogadro's number :
Avogadro's number is approximately 6.022 ∗ 1 0 23 a t o m s / m o l .
Calculate the number of silver atoms in the bar:
Number of atoms = Moles x Avogadro's number
Number of atoms = 9.73 m o l es ∗ 6.022 ∗ 1 0 23 a t o m s / m o l ≈ 5.86 ∗ 1 0 24 a t o m s
Thus, there are approximately 5.86 ∗ 1 0 24 a t o m s of silver in the 100 mL silver bar.
For more such questions on silver:
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Answered by anuradhaborua | 2024-06-18

In a 100 mL silver bar with a density of 10.5 g/mL, there are approximately 5.86 × 1 0 24 atoms of silver. This is calculated by first determining the mass of the silver, then calculating the moles, and finally using Avogadro's number to find the total number of atoms. The steps involve basic formulas in chemistry, particularly related to mass, moles, and atomic count.
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Answered by anuradhaborua | 2024-12-26