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Chapter 12: Problem 17

Butanol and pentane have approximately the same mass, however, the viscosity (at \(20^{\circ} \mathrm{C}\) ) of butanol is \(\eta=2.948 \mathrm{cP},\) and the viscosity of pentane is \(\eta=0.240 \mathrm{cP.}\) Explain this difference.

Short Answer

Expert verified
The difference in viscosity is due to the different kinds of intermolecular forces present in Butanol and Pentane. Butanol, having Hydrogen bonds, a stronger form of intermolecular force, has higher viscosity as compared to Pentane, which only has the weaker Van der Waals' forces.

Step by step solution

01

Understanding Molecular Structure

In molecular terms, viscosity can be attributed to the intermolecular forces between the individual particles of a substance. Both Butanol and Pentane are hydrocarbon compounds, meaning they are composed only of Hydrogen and Carbon atoms. However, their structural difference is crucial. Butanol is an alcohol with a single bonded Oxygen atom which leads to the formation of Hydrogen bonds between the Butanol molecules, while Pentane is an alkane which only has Van der Waals' forces.
02

Understanding Intermolecular Forces

Hydrogen bonding, which occurs in Butanol, is a stronger intermolecular force than the Van der Waals' forces in Pentane. These stronger forces in Butanol lead to an increase in resistance to flow, hence a higher viscosity. Conversely, the weaker Van der Waals' forces in Pentane result in lesser resistance to flow, hence a lower viscosity.
03

Conclusion

Therefore, despite the similar mass of Butanol and Pentane, their viscosities differ due to the nature of the intermolecular forces present within each substance. The presence of Hydrogen bonds in Butanol, a stronger type of intermolecular force, results in a higher viscosity when compared to Pentane, which only experiences Van der Waals' forces.

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