Answer:
1.71 × 10²⁵ atoms
Step-by-step explanation:
A pure titanium cube has an edge length of 2.64 in. In centimeters,
2.64 in × (2.54 cm/ 1 in) = 6.71 cm
The volume of the cube is:
V = (length)³ = (6.71 cm)³ = 302 cm³
Titanium has a density of 4.50 g/cm³. The mass corresponding to 302 cm³ is:
302 cm³ × 4.50 g/cm³ = 1.36 × 10³ g
The molar mass of titanium is 47.87 g/mol. The moles corresponding to 1.36 × 10³ g are:
1.36 × 10³ g × (1 mol/47.87 g) = 28.4 mol
1 mol of Ti contains 6.02 × 10²³ atoms of Ti (Avogadro's number). The atoms in 28.4 moles are:
28.4 mol × (6.02 × 10²³ atoms/1 mol) = 1.71 × 10²⁵ atoms