Answer:
Step-by-step explanation:
3. We know the aluminum can has a mass of 12.8 g. We need moles of Al.
1 can = 12.8 g
1 mol Al = 27.0 g Al
12.8 g Al x (1 mol Al/27.0 g) = 0.474 mol
Note: The units of gram cancel and we are left with moles.
4. We have the mass of the can at 12.8 g. We need to use molar mass and Avogadro's number to find atoms.
1 mole = 6.022 x 10²³ atoms
12.8 g Al x (1 mol Al/27.0 g Al) x [(6.022 x 10²³/1 mol)] = 2.95 x 10²³ atoms
Note: The units of g and mol cancel and you are left with atoms.
5. Now we need to know how many cans it takes to have 1 mole of aluminum.
1 mol Al x (27.0 g Al/1 mol Al) x (1 can Al/12.8 g Al) = 2.11 cans
Note: The g and mol cancel and you are left with can.