okay so i'm doing a chemistry lab where we were given a sheet of aluminum foil and have to calculate how many atoms thick the sheet isright now, we are learning about moles and conversion factorsmy teacher said conversion factors were key to answering the labI have no idea what to do or how to do itplease help me.below is information i have gathered.size of my sheet: 8mm by 7mmhow many moles in my sheet? 0.008524 molesmolar mass of aluminum: 26.9815386 g/molweight of the entire roll of aluminum foil: 100.20 gramsweight of my sheet: 0.23 gramsthis is all i have, please help me! remember he said to use conversion factors if that helpsand i think moles can represent an atomthanks,mason
Don't worry, since you're not regular there won't be any patternJust let it be for a bit longer and things will settle down soon ;)
one mole is an avagadro's number of atoms: 6.0221413e+23 Do you know the density of the aluminum in g/cm3 ? If so, you could easily figure out the actual volume of the sheetFrom that you could find the thickness of your sheetSince you know the total number of atoms (from the number of moles) you could determine the relative volume of an atom, and assume that they are either balls or cubes and figure out the thickness using radius of the atomsBut I am not sure if you have enough information above to figure this outIf you knew the volume of the atoms, or the density of the material, or even just the thickness of the foil in mm then you could figure it outGood luck
