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Chapter 7: Problem 20

Water vapor liquefies when cooled below \(100^{\circ} \mathrm{C}\). Gaseous nitrogen liquefies when cooled below \(-196^{\circ} \mathrm{C}\). What does this information tell you about the relative strengths of the intermolecular forces for these molecules?

Short Answer

Expert verified
The given information indicates that the intermolecular forces in water vapor are stronger than those in gaseous nitrogen, as water vapor has a higher liquefaction temperature (\(100^{\circ} \mathrm{C}\)) compared to gaseous nitrogen (\(-196^{\circ} \mathrm{C}\)).

Step by step solution

01

Identify the given information

The liquefaction temperatures for water vapor and gaseous nitrogen are given as \(100^{\circ} \mathrm{C}\) and \(-196^{\circ} \mathrm{C}\) respectively.
02

Compare the liquefaction temperatures

Water vapor liquefies at \(100^{\circ} \mathrm{C}\), which is higher than the liquefaction temperature of gaseous nitrogen, \(-196^{\circ} \mathrm{C}\).
03

Relate the liquefaction temperatures to intermolecular forces

Since water vapor has a higher liquefaction temperature than gaseous nitrogen, it means that the intermolecular forces in water vapor are stronger than those in gaseous nitrogen.
04

State the conclusion

The given information tells us that the intermolecular forces in water vapor are stronger than those in gaseous nitrogen, as indicated by the higher liquefaction temperature of water vapor compared to gaseous nitrogen.

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