Answer: C2H6O2
Explanation: solution attached:
First convert mass to moles.
Second divide each moles on the lowest amount to find the number of atoms in the empirical formula.
Third calculate the empirical formula mass.
Fourth calculate for the molecular formula by dividing the molar mass over the empirical formula mass.
Fifth multiply the empirical formula by the answer and that is the molecular formula of the compound.
In the given case of a sample (3.585g) contain 1.388g of C, 0.345g of H, 1.850g of O, and its molar mass is 62g, the molecular formula of this substance - C2H6O2
To get the molecular formula we need to find the empirical formula first. To get empirical we need to follow these steps:
1. convert mass to moles.
moles C = = 0.116 mol
moles H = = 0.345 mol
moles O = = 0.116 mol
2. divide each mole on the lowest amount to find the number of atoms in the empirical formula.
C = [tex]\frac{0.116}{0.116}[/tex] = 1
H = [tex]\frac{0.345}{0.116}[/tex] = 3
O = [tex]\frac{0.116}{0.116}[/tex] = 1
3. calculate the empirical formula mass
Empirical formula = CH3O
4. calculate the molecular formula by dividing the molar mass over the empirical formula mass.
ratio = 62/31 = 2
this only has a molecular weight of 31 g/mol, but we are told the molecular weight is 62 g/mol. Therefore, we just multiply the number of each atom by 2 giving us the following molecular formula:
Molecular formula = 2(CH3O) = C2H6O2
Thus, In the given case of a sample (3.585g) contain 1.388g of C, 0.345g of H, 1.850g of O, and its molar mass is 62g, the molecular formula of this substance - C2H6O2
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