How many atoms think is a sheet of aluminum foil? Which measurements are critical to solve this problem?
NoYou can't legally make a pass over a double yellow lineAnd the fact that you didn't know that, but STILL are on the road driving is very distressing.
Believe it or not, you can find the thickness of the foil by determining its volumeThen by knowing the area you can find the thicknessNow gold is much more malleable and it can be beaten to a thickness of about 1 atomThis was used in the experiments to measure the sizes of particles by Rutherford, I thinkBut you aren't getting near that in aluminum foilSo, find the density of the foil and the area of the sheetSay that you know the area and the density, and you multiply them, you will get an answer of: [m^2][g/m^3] g/mFind the number of grams in a mole of Al, then divide Avogadro's number by this ratio: [Mole/g][atoms/Mole] [atoms/g] Next, multiply your first answer by the second and you get a fairly accurate answer[g/m][atoms/g] [atoms/m] Remember, that not all Al atoms are the same size, and there are crystals and impurities in the AlBut unless you are in Physical Chemistry studying the inner workings of the atom this should work.
