The boiling point of cycloalkanes is generally higher than their corresponding linear alkanes with the same number of carbons. This trend can be explained by considering the factors that influence boiling points: molecular weight, molecular shape, and intermolecular forces.1. Molecular weight: In this case, both cycloalkanes and linear alkanes have the same number of carbons, so their molecular weights are similar. This factor does not contribute to the difference in boiling points.2. Molecular shape: Cycloalkanes have a cyclic structure, which makes them more compact and less elongated compared to linear alkanes. This difference in shape affects the surface area available for intermolecular interactions.3. Intermolecular forces: The primary intermolecular forces in both cycloalkanes and linear alkanes are van der Waals forces also known as London dispersion forces . These forces are influenced by the surface area available for interactions between molecules. Since cycloalkanes have a more compact structure, their molecules can pack more closely together, leading to stronger van der Waals forces compared to linear alkanes.The stronger van der Waals forces in cycloalkanes result in a higher boiling point compared to their corresponding linear alkanes with the same number of carbons. This is because more energy is required to overcome these stronger intermolecular forces and convert the cycloalkane from a liquid to a gas.