## Molecular to Empirical [ENDORSED]

Sunjum Singh 1I
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Joined: Fri Apr 06, 2018 11:05 am

### Molecular to Empirical

When given the Molecular Formula, how do you find the empirical from it? A somewhat similar example is F.26 in the homework. Thanks.

Susu Le 1F
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### Re: Molecular to Empirical

You should divide the number of atoms for each element in the molecular formula by the greatest number that would still leave you with whole numbers. For example the molecular formula for glucose is C6H12O6. Dividing this by 6 would still give you whole numbers: CH2O. This is the empirical formula for glucose.

Caitlyn Ponce 1L
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### Re: Molecular to Empirical

Molecular formulas are multiples of empirical formulas. In order to get the empirical formula from the molecular formula, you need to reduce the molecular formula to its simplest whole number ratio of atoms. For example, butane has the molecular formula C4H10. We divide by 2 to reduce it and the resulting empirical formula is C2H5.

Gisselle Sainz 2F
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Joined: Wed Feb 21, 2018 3:00 am

### Re: Molecular to Empirical

To go from molecular to empirical formula you divide the subscripts of the molecular formula by the greatest common divisor to get the most reduced form of the formula which is essentially the empirical formula.

YeseniaGomez_1L
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### Re: Molecular to Empirical

It is basically just like simplifying in math. Once you have the molecular formula you simplify using the greatest common number that you can divide by. For example lets say we have C6H12, then you can simplify by dividing what you have by 6 since both numbers are divisible by 6 to get CH6. Don't forget it is also possible for the molecular and empirical formulas to be the same so if you get a molecular formula that seems can not be simplified further, that should also be your empirical formula.

Bijal Luhar
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Joined: Fri Apr 06, 2018 11:03 am

### Re: Molecular to Empirical

To go from molecular formula to empirical formula you basically divide by the greatest common factor of all the elements. Remember that empirical formulas are ratios of the molecular. For example, C10H20O5 the greatest common factor of 10,20,and 5 is 5. So you divide all those coefficients by 5 and get c2h4o!

Vienna Cimetta 1L
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Joined: Thu Feb 01, 2018 3:01 am

### Re: Molecular to Empirical

Also just as a side note, if visual diagram of the compound is given often it's easier to start by naming the molecular formula, then reduce the numbers to the empirical formula. I assume if one of the elements is only present once the empirical formula would be the same, since you have to only have whole numbers.

005006577
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Joined: Fri Apr 06, 2018 11:02 am

### Re: Molecular to Empirical

When presented with just a molecular formula, the empirical formula can be found by dividing by the greatest whole number that each element is divisible by. However, if the molecular formula is not able to be divided by any number, the empirical formula is known to be the same as the molecular formula.

juliaschreib1A
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Joined: Fri Sep 29, 2017 7:06 am

### Re: Molecular to Empirical

Just divide by a common denominator to get the empirical formula.

Posts: 27
Joined: Fri Apr 06, 2018 11:04 am

### Re: Molecular to Empirical

In a typical "finding the molecular formula problem," is there a way to discover the molecular formula before the empirical formula, in order to save critical time during an examination?

Yuliana Garcia 1a
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Joined: Fri Apr 06, 2018 11:02 am

### Re: Molecular to Empirical

We can obtain the empirical formula through the molecular formula, by dividing by its highest common denominator. Due to the fact that the molecular is the actual number of atoms, while the empirical is the relative number of atoms.

MariaJohn1D
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Joined: Wed Nov 08, 2017 3:01 am

### Re: Molecular to Empirical

To go from the molecular formula to the empirical formula you should divide by the greatest common denominator. Please keep in mind that the molecular and empirical formula can be the same.

Chem_Mod
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### Re: Molecular to Empirical  [ENDORSED]

There is no way to find the molecular formula before finding the empirical formula unless the molecular formula is given to you initially.