A 25.0mm*40.0mm PIECE OF GOLD FOIL IS 0.25mm THICK. THE DENSITY OF GOLD IS 19.32g/(cm)3
HOW MANY GOLD ATOMS ARE IN SHEET ?
The first thing to do here is to figure out the volume of the foil.
V= length of foil x width of of foil x thickness or height of foil
Density of gold is in grams per cubic centimeter, g cm−3.
We know,
1 cm = 10 mm
The volume of the foil,
V=(40.0mmx1 cm/10mm)x(25.0mmx1 cm/10mm)x(0.25mmx1 cm/10mm)
V=0.25 cm3
Mass of the foil using density of gold,
0.25cm3x19.32 g/1cm3=4.83 g
The number of atoms of gold present in this sample, you must convert the number of grams to moles by using the element's molar mass
4.83g x 1 mole Au/196.97g=0.02452 moles Au
Use Avogadro's constant, i.e. the definition of a mole, to convert the number of moles to number of atoms
0.02452moles Au x 6.022⋅1023.atoms of Au / 1 mole Au
=1.5 x 1022 atoms of Au
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