Ranking the Boiling Points of CO2, CS2, and CSe2

What is the correct ranking of the normal boiling points of CO2, CS2, and CSe2 from the lowest to the highest?

CO2 < CS2 < CSe2

Explanation:

The boiling points of CO2, CS2, and CSe2 increase with their molecular weight. The normal boiling point of a substance is determined by several factors, with molecular weight playing a significant role. In this case, carbon dioxide (CO2), carbon disulfide (CS2), and carbon diselenide (CSe2) are compared based on their boiling points. CO2 has the lowest boiling point among the three compounds. It has the least molecular weight, resulting in weaker intermolecular forces which require less energy to break the bonds and transition from a liquid to a gas state. On the other hand, CSe2 has the highest boiling point as it has the highest molecular weight among the three. The stronger London dispersion forces in CSe2 contribute to a higher boiling point compared to CO2 and CS2. Therefore, the correct ranking of the boiling points of CO2, CS2, and CSe2 is CO2 < CS2 < CSe2.
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