The boiling point for species A at 1 bar is reported to be 250 K, and you desire

Question

The boiling point for species A at 1 bar is reported to be 250 K, and you desire to know the boiling point at 10 bar. Knowing the enthalpy of vaporization, you apply the Clausius-Clapeyron equation and calculate the temperature to be 300 K. However, at that pressure, you also know that species A is not an ideal gas, but rather attractive intermolecular interactions are significant. If you accounted for the attractive interactions, you would find that Species A boils (at less than 300 K, at 300 K, at greater than 300 K, or there is no way to determine). Explain your answer.

Explanation / Answer

Assuming the gas a to be ideal gas , we calculated its boiling point at 10 bar to be 300K. Now that we know , A is not an ideal gas and hassignificant attractive inter molecular forces , the boiling temperature of species A has to be greater than 300K.

It can be explained as, more intermolecular attractions, more energy required to separate the molecules . Thus more heat to be supplied increasing the boiling point.

In liquid state the intermolecular attractions are much greater than in gaseous state.

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