The empirical formula of a compound is the lowest whole-number ratio of atoms in the compound. The molecular formula gives the actual number of each type of atom in a molecule. For example, the compound `N_2O_2` has the empirical formula NO.
The molar mass of a compound is a whole-number multiple of its empirical formula mass.
Let's start by finding the empirical formula mass of this compound:
`CH_2O` = C + (2)H + O =...
The empirical formula of a compound is the lowest whole-number ratio of atoms in the compound. The molecular formula gives the actual number of each type of atom in a molecule. For example, the compound `N_2O_2` has the empirical formula NO.
The molar mass of a compound is a whole-number multiple of its empirical formula mass.
Let's start by finding the empirical formula mass of this compound:
`CH_2O` = C + (2)H + O = 12.0 + 2(1.0) + 16.0= 30 grams per mole
We can find the factor by which the molecular formula is larger than the empirical formula by comparing the two masses. Divide the actual molar mass of the compound by the empirical formula mass:
120/30 = 4
Since the molar mass of the compound is four times the empirical formula mass, the molecular formula is four times the empirical formula:
`4(CH_2O)` = `C_4H_8O_2`
The linked video provides a detailed explanation and some more examples of this process.
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