Final answer:
To find the number of atoms in samples of copper and copper (I) sulfate, we apply the molar mass of copper and Avogadro's number. The calculations show how many copper atoms are present in 2 moles of copper, 2 grams of copper, 2 moles of copper (I) sulfate, and 2 grams of copper (I) sulfate.
Step-by-step explanation:
To calculate the number of atoms in various copper samples and compounds, we use the molar mass of copper and Avogadro's number. The atomic mass of copper (Cu) is approximately 63.55 g/mol, and Avogadro's number (NA) is 6.022 × 1023 atoms per mole.
For 2 moles of Cu:
- 2 moles × 6.022 × 1023 atoms/mole = 1.2044 × 1024 Cu atoms
For 2 g of Cu:
- (2 g Cu) / (63.55 g/mol) = 0.0315 moles Cu
- 0.0315 moles × 6.022 × 1023 atoms/mole = 1.8969 × 1022 Cu atoms
To calculate for copper (I) sulfate (Cu2SO4), we first need the molar mass of this compound which is approximately 223.15 g/mol for Cu2SO4.
For 2 moles of copper (I) sulfate:
- 2 moles × 6.022 × 1023 molecules/mole × 3 atoms/molecule of Cu = 3.6132 × 1024 Cu atoms (each molecule has 3 Cu atoms)
For 2 g of copper (I) sulfate:
- (2 g Cu2SO4) / (223.15 g/mol) = 0.00896 moles of Cu2SO4
- 0.00896 moles × 6.022 × 1023 molecules/mole × 3 atoms/molecule of Cu = 1.6181 × 1022 Cu atoms
Note: The 'molecules/mole' unit in the above calculations for copper (I) sulfate denotes the relationship between moles of compound and the number of molecules. Each copper (I) sulfate molecule contains 3 Cu atoms.