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Chapter 10: Problem 14

The nonpolar hydrocarbon \(\mathrm{C}_{25} \mathrm{H}_{52}\) is a solid at room temperature. Its boiling point is greater than \(400^{\circ} \mathrm{C} .\) Which has the stronger intermolecular forces, $\mathrm{C}_{25} \mathrm{H}_{52}\( or \)\mathrm{H}_{2} \mathrm{O}$ ? Explain.

Short Answer

Expert verified
\(\mathrm{C}_{25}\mathrm{H}_{52}\) has stronger intermolecular forces than \(H_2O\). Although hydrogen bonding in \(H_2O\) is generally stronger than London dispersion forces, the large size of \(\mathrm{C}_{25}\mathrm{H}_{52}\) results in stronger London dispersion forces, leading to a higher boiling point compared to water.

Step by step solution

01

Identify the types of intermolecular forces present in each substance

First, we need to identify the types of intermolecular forces that exist in both substances. In \(\mathrm{C}_{25}\mathrm{H}_{52}\), a nonpolar hydrocarbon, the intermolecular force present is London dispersion forces (also known as van der Waals forces). In water, \(H_2O\), there are two types of intermolecular forces: hydrogen bonding (a strong type of dipole-dipole interaction) and London dispersion forces.
02

Compare the boiling points of the substances

Given that the boiling point of \(\mathrm{C}_{25}\mathrm{H}_{52}\) is greater than \(400^{\circ} \mathrm{C}\) and the boiling point of \(H_2O\) is \(100^{\circ} \mathrm{C}\), it seems that \(\mathrm{C}_{25}\mathrm{H}_{52}\) has stronger intermolecular forces. However, we must also consider that \(\mathrm{C}_{25}\mathrm{H}_{52}\) has a much larger molecular weight compared to \(H_2O\). Thus, it also has more electrons which leads to stronger London dispersion forces.
03

Analyze the strength of the intermolecular forces

We know that hydrogen bonding in \(H_2O\) is a stronger intermolecular force than London dispersion forces. However, due to the large size of \(\mathrm{C}_{25}\mathrm{H}_{52}\), the London dispersion forces experienced by the hydrocarbon are strong enough to result in a higher boiling point compared to water.
04

Conclusion

Even though hydrogen bonding is generally stronger than London dispersion forces, the large size of \(\mathrm{C}_{25}\mathrm{H}_{52}\) results in stronger London dispersion forces than those experienced by \(H_2O\). Hence, \(\mathrm{C}_{25}\mathrm{H}_{52}\) has stronger intermolecular forces compared to \(H_2O\).

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