Copper crystallizes in a face centered cubic lattice . Calculate the nmber of unit cell in 1.2 g of copper atomic mass of copper is 63.5 u
fcc has 4 atoms per unit cell
6.02E23 amu per gram
(1.2 * 6.02E23) / (63.5 * 4)
To find the number of unit cells in 1.2 g of copper, we can use the following steps:
Step 1: Determine the number of moles of copper.
Since we know the atomic mass of copper is 63.5 u, we can calculate the number of moles using the formula:
Number of moles = Mass / Molar mass
Mass = 1.2 g
Molar mass = 63.5 g/mol
Number of moles = 1.2 g / 63.5 g/mol
Step 2: Calculate the number of atoms per unit cell.
In a face-centered cubic (FCC) lattice, there are 4 atoms per unit cell. This is a characteristic of the crystal structure of copper.
Step 3: Find the Avogadro's number.
Avogadro's number (Nᴀ) is the number of atoms or molecules in one mole of a substance. It is approximately 6.022 × 10^23.
Step 4: Determine the number of unit cells.
To find the number of unit cells, we need to divide the number of atoms in the sample by the number of atoms per unit cell:
Number of unit cells = Number of moles × Avogadro's number / Number of atoms per unit cell
Let's plug in the values:
Number of unit cells = (1.2 g / 63.5 g/mol) × (6.022 × 10^23) / 4
Now, you can solve this equation to find the number of unit cells in 1.2 g of copper.