The enthalpy of fusion of water is 6.0 kJ/molrxn and that of methanol (CH3OH) is 3.2 kJ/molrxn.
Which solid, water or methanol, has the larger intermolecular forces?
Predict whether the enthalpy of fusion of C2H6 will be larger than, less than, or the same of that of methanol.
Water seems to require more energy to break apart the bonds caused by intermolecular forces.
thank you
*This is the second part of the question
Predict whether the enthalpy of fusion of C2H6 will be larger than, less than, or the same of that of methanol.
What do you remember about hydrogen bonding. That's present in the water. Could it also be present in CH3OH?
It would be less than that of methanol
I agree.
To determine which solid, water or methanol, has the larger intermolecular forces, we need to consider the types of intermolecular forces present in each substance.
Water is a polar molecule, meaning it has an uneven distribution of charge due to the presence of oxygen with a partial negative charge and hydrogen with partial positive charges. This polarity allows water to form hydrogen bonds, which are stronger intermolecular forces compared to other types of forces. As a result, water has relatively strong intermolecular forces.
Methanol, on the other hand, also has polar molecules due to the presence of oxygen, but it has weaker intermolecular forces than water. Methanol can form hydrogen bonds as well, but not to the same extent as water.
Based on this information, it can be concluded that water has larger intermolecular forces compared to methanol.
To predict whether the enthalpy of fusion of C2H6 (ethane) will be larger than, less than, or the same as that of methanol, we need to analyze the types of intermolecular forces present in each substance.
Ethane (C2H6) is a nonpolar molecule, meaning it has no significant charge separation. Therefore, ethane can only form London dispersion forces, which are generally weaker than hydrogen bonds.
Methanol, as mentioned before, is a polar molecule that can form hydrogen bonds.
Since hydrogen bonds are stronger intermolecular forces compared to London dispersion forces, it can be predicted that methanol has a larger enthalpy of fusion than ethane.