Determining the Number of Atoms for the Empirical Formula
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Determining the Number of Atoms for the Empirical Formula
Once you divide the each of the number of moles of each type of atom by the smallest value you usually get a whole number right away. But I was wondering what to do if you get a number that is slightly off, for example if you get 4.03 is it okay to use 4 for the number of atoms in the empirical formula? I know if you get 1.33, for example, you should multiply by 3 to get a whole, but in the case of a number like 4.03 it doesn't really make sense to multiply, so should I just use 4?
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Re: Determining the Number of Atoms for the Empirical Formula
Yeah if it’s very close to a whole number you don’t have to worry about it. 4.03 is close enough to 4!
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Re: Determining the Number of Atoms for the Empirical Formula
Yes, when a number can be rounded from the hundredth's place it is okay to round up or down to a whole number (ex: 4.03 can be rounded to 4, and 3.98 can be rounded to 4). However if a number can't be rounded from the hundredth's place to reach a whole number, then it should be multiplied by a factor to get the smallest whole number possible. (ex: 2.5 can't be rounded so you would multiply by a factor of 2 to get 5)
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