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A piece of copper has a mass of 820 g. How many atoms does the sample contain?

User Dwsolberg
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Answer:

To determine the number of atoms in a sample of copper, we need to use the concept of molar mass and Avogadro's number. Here's a step-by-step guide on how to calculate it:

1. Find the molar mass of copper. The molar mass represents the mass of one mole of a substance. The atomic mass of copper is approximately 63.55 g/mol.

2. Convert the mass of the sample to moles. To do this, divide the mass of the sample (820 g) by the molar mass of copper (63.55 g/mol):

Number of moles = Mass of sample / Molar mass

= 820 g / 63.55 g/mol

3. Calculate the number of atoms in the sample using Avogadro's number. Avogadro's number is approximately 6.022 x 10^23 atoms/mol.

Number of atoms = Number of moles x Avogadro's number

= (820 g / 63.55 g/mol) x (6.022 x 10^23 atoms/mol)

4. Perform the calculation to find the number of atoms in the sample:

Number of atoms = (820 g / 63.55 g/mol) x (6.022 x 10^23 atoms/mol)

Make sure to carry out the multiplication and division correctly using a calculator or spreadsheet software.

By following these steps, you can calculate the number of atoms in the sample of copper.

Step-by-step explanation:

User Venessa
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