Now that you have predicted the boiling points of the compounds, try to rotate t

Question

Now that you have predicted the boiling points of the compounds, try to rotate the boiling point to the compound's volatility which describes how high its vapor pressure compounds that are very volatile escape into the gas phase easily and you can smell them! The vapor pressure curves for carbon disulfide (CS_2) and nitro methane(CH_3NO_2) are drawn below. What are their normal boiling points? What are the approximate vapor pressures of each compound at 40 degree C? Each person should write down an explanation (in their own words) of how the intermolecular interactions result in this difference in volatility. As a group, read through the explanations and see how different people understand this phenomena. Write a revised version that is concise, but complete.

Explanation / Answer

The liquid which having low vapour pressure or low volatile liquid is having high boiling point.

The liquid which having high vapour pressure or high volatile liquid is having low boiling point.

As we can see in figure, at a particular temperature CS2 is having more vapour pressure than nitromethane. Therefore, CS2 is more volatile and having less boiling point.

The temperature at which vapour pressure of a liquid is 760 mm, then that temp. is called boiling point to that liquid

By figure, we can say approximately, CS2 boiling point is about 45 oC and CH3NO2 boiling point is about 100 oC.

At 40 oC, CS2 vapour pressure is about 600 torr and CH3NO2 vapour pressure is about 20-25 torr.

Best wishes.

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