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Molecular formulas:
- CH₂O;
- C₂H₄O₂;
- C₆H₁₂O₆.
The empirical formula of a compound tells only the ratio between atoms of each element. The empirical formula CH₂O indicates that in this compound,
- for each C atom, there are
- two H atoms, and
- one O atom.
The molecular weight (molar mass) of the molecule depends on how many such sets of atoms in each molecule. The empirical formula doesn't tell anything about that number.
It's possible to <em>add</em> more of those sets of atoms to a molecular formula to increase its molar mass. For every extra set of those atoms added, the molar mass increase by the mass of that set of atoms. The mass of one mole of C atoms, two mole of H atoms, and one mole of O atoms is .
- CH₂O- 30.0 g/mol;
- C₂H₄O₂- 30.0 + 30.0 = 2 × 30.0 = 60.0 g/mol;
- C₃H₆O₃- 30.0 + 30.0 + 30.0 = 3 × 30.0 = 90.0 g/mol.
It takes one set of those atoms to achieve a molar mass of 30.0 g/mol. Hence the molecular formula CH₂O.
It takes two sets of those atoms to achieve a molar mass of 60.0 g/mol. Hence the molecular formula C₂H₄O₂.
It takes sets of those atoms to achieve a molar mass of 180.0 g/mol. Hence the molecular formula C₆H₁₂O₆.
To develop this problem it is necessary to use the concepts related to Impulse.
The impulse is defined as the change in velocity at the rate of mass, that is
Where,
m = Mass
Change in Velocity
This change in velocity can be expressed as,
Therefore the magnitude of the impulse is 4.32 Kg.m/s