calculation of molecular formula mass formula
Answers
Answer:
Below, we see two carbohydrates: glucose and sucrose. Sucrose is almost exactly twice the size of glucose, although their empirical formulas are very similar. Some people can distinguish them on the basis of taste, but it's not a good idea to go around tasting chemicals. The best way is to determine the molar masses—this approach allows you to easily tell which compound is which.
Molecular Formulas
Molecular formulas give the kind and number of atoms of each element present in the molecular compound. In many cases, the molecular formula is the same as the empirical formula. The chemical formula will always be some integer multiple ( n ) of the empirical formula (i.e. integer multiples of the subscripts of the empirical formula).
Molecular Formula=n(Empirical formula)(6.9.1)
therefore
n=Molecular FormulaEmpirical Formula(6.9.2)
The integer multiple, n, can also be obtained by dividing the molar mass, MM , of the compound by the empirical formula mass, EFM (the molar mass represented by the empirical formula).
n=MM(molarmass)EFM(empiricalformulamolarmass)(6.9.3)
n=
Answer:
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Explanation:
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