CH3(CH2)2CH3 (butane) 58.1 -0.5 CH3COCH3 (acetone) 58.1 56.2 a)Identify all intermolecular forces present in a pure sample of these compounds. b)Explain the difference in boiling points of these three compounds. c)Which substance will have
| Compound | Molar Mass (g/mol) | Boiling point (degrees C) |
| CH3CH2CH2OH (1-propanol) | 60.1 | 97 |
| CH3(CH2)2CH3 (butane) | 58.1 | -0.5 |
| CH3COCH3 (acetone) | 58.1 | 56.2 |
a)Identify all intermolecular forces present in a pure sample of these compounds.
b)Explain the difference in boiling points of these three compounds.
c)Which substance will have the highest vapor pressure?
1)In propanol, there is presence of oxygen bond which is electronegative in nature.It will attract the electron towards itself hence generating a dipole. And Oxygen is further attached with hydrogen which will result into hydrogen bonding.In a sample there are so many molecules are present hence intermolecular hydrogen bonding can also takes place. hence there will be dipole-dipole attraction and hydrogen bonding.
2)In butane there is no electronegative atom present. there is no dipole as it is a non polar molecule. it has london dispersive forces of attraction.
3)In acetone, C and O have difference in electronegativity there will be generation of dipole as oxygen will attract the electron density towards itself. There will be dipole dipole interaction only.
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