Water (H2O) and methane (CH4) are simple compounds with covalent bonds and a similar molecular mass.
In theory, this should mean that they share similar physical and chemical properties however, this is not the case.
The table below compares some of the features of methane and water:
Water | Methane | |
Molecular weight | 18 | 16 |
Latent heat of vaporisation / kJ kg-1 | 2 260 | 510 |
Specific heat capacity / kJ kg-1 °C-1 | 4.2 | 2.2 |
Melting point / °C | 0 | -182 |
Boiling point / °C | 100 | -162 |
Which of the statements below correctly describes the reason for these property differences?
Water is able to form hydrogen bonds with adjacent water molecules.
Methane forms a tetrahedral structure due to the fact carbon is able to form four covalent bonds.
Methane has a higher energy content in its bonds than water.
Water has a higher density than methane in a liquid state.
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