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Chapter 11: Problem 46

True or false: (a) \(\mathrm{CBr}_{4}\) is more volatile than \(\mathrm{CCl}_{4}\). (b) \(\mathrm{CBr}_{4}\) has a higher boiling point than \(\mathrm{CCl}_{4}\). (c) \(\mathrm{CBr}_{4}\) has weaker intermolecular forces than \(\mathrm{CCl}_{4}\). (d) \(\mathrm{CBr}_{4}\) has a higher vapor pressure at the same temperature than \(\mathrm{CCl}_{4}\)

Short Answer

Expert verified
(a) False (b) True (c) False (d) False

Step by step solution

01

Understanding Volatility

Volatility is the ability of a substance to evaporate or turn into a vapor at a given temperature. In general, substances with weaker intermolecular forces tend to have higher volatility as less energy is required to separate the molecules. To determine whether \(\mathrm{CBr}_{4}\) is more volatile than \(\mathrm{CCl}_{4}\), we need to compare their intermolecular forces.
02

Comparing Intermolecular Forces

The dominant intermolecular forces between \(\mathrm{CBr}_{4}\) and \(\mathrm{CCl}_{4}\) are London Dispersion Forces (LDF), which are temporary attractive forces that result from the constant motion of electrons. LDFs are stronger in molecules with more electrons, as they have larger electron clouds which can create stronger temporary dipoles. Since bromine has more electrons than chlorine, \(\mathrm{CBr}_{4}\) has stronger LDFs than \(\mathrm{CCl}_{4}\).
03

Answering Statement (a)

Since \(\mathrm{CBr}_{4}\) has stronger LDFs than \(\mathrm{CCl}_{4}\), it will require more energy to separate the molecules and is therefore less volatile. Statement (a) is false.
04

Understanding Boiling Points

The boiling point of a substance is the temperature at which its vapor pressure equals atmospheric pressure. In general, substances with stronger intermolecular forces have higher boiling points, as more energy is required to separate the molecules and overcome the attractive forces.
05

Answering Statement (b)

Since \(\mathrm{CBr}_{4}\) has stronger LDFs than \(\mathrm{CCl}_{4}\), it will have a higher boiling point. Statement (b) is true.
06

Answering Statement (c)

We already established that \(\mathrm{CBr}_{4}\) has stronger LDFs than \(\mathrm{CCl}_{4}\). Statement (c) is false.
07

Understanding Vapor Pressure

Vapor pressure is the pressure exerted by a vapor in equilibrium with its liquid phase at a given temperature. Substances with higher volatility have higher vapor pressures, as they evaporate more readily.
08

Answering Statement (d)

Since \(\mathrm{CBr}_{4}\) is less volatile than \(\mathrm{CCl}_{4}\) due to its stronger LDFs, it will have a lower vapor pressure at the same temperature. Statement (d) is false.

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Most popular questions from this chapter

When an atom or group of atoms is substituted for an atom in benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)\), the boiling pointchanges. Explair the order of the following boiling points: \(\mathrm{C}_{6} \mathrm{H}_{6}\left(80^{\circ} \mathrm{C}\right)\) \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{Cl}\left(132{ }^{\circ} \mathrm{C}\right), \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{Br}\left(156^{\circ} \mathrm{C}\right), \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{OH}\left(182{ }^{\circ} \mathrm{C}\right) .\)

Appendix B lists the vapor pressure of water at various external pressures. (a) Plot the data in Appendix \(B\), vapor pressure (torr) vs. temperature \(\left({ }^{\circ} \mathrm{C}\right)\). From your plot, estimate the vapor pressure of water at body temperature, \(37^{\circ} \mathrm{C}\). (b) Explain the significance of the data point at \(760.0\) torr, \(100^{\circ} \mathrm{C}\) (c) A city at an altitude of \(5000 \mathrm{ft}\) above sea level has a barometric pressure of 633 torr. To what temperature would you have to heat water to boil it in this city? (d) A city at an altitude of \(500 \mathrm{ft}\) below sea level would have a barometric pressure of 774 torr. To what temperature would you have to heat water to boil it in this city? (e) For the two cities in parts (c) and (d), compare the average kinetic energies of the water molecules at their boiling points. Are the kinetic energies the same or different? Explain.

The critical temperatures (K) and pressures (atm) of a series of halogenated methanes are as follows: $$ \begin{array}{lllll} \hline \text { Compound } & \mathrm{CCl}_{3} \mathrm{~F} & \mathrm{CCl}_{2} \mathrm{~F}_{2} & \mathrm{CClF}_{3} & \mathrm{CF}_{4} \\ \hline \text { Critical Temperature } & 471 & 385 & 302 & 227 \\ \text { Critical Pressure } & 43.5 & 40.6 & 38.2 & 37.0 \\ \hline \end{array} $$ (a) List the intermolecular forces that occur for each compound. (b) Predict the order of increasing intermolecular attraction, from least to most, for this series of compounds. (c) Predict the critical temperature and pressure for \(\mathrm{CCl}_{4}\) based on the trends in this table. Look up the experimentally determined critical temperatures and pressures for \(\mathrm{CCl}_{4}\), using a source such as the \(\mathrm{CRC}\) Handbook of Chemistry and Physics, and suggest a reason for any discrepancies.

For each of the following pairs of substances, predict which will have the higher melting point, and indicate why: (a) HF, \(\mathrm{HCl} ;\) (b) C (graphite), \(\mathrm{CH}_{4}\); (c) \(\mathrm{KCl}, \mathrm{Cl}_{2}\); (d) \(\mathrm{LiF}, \mathrm{MgF}_{2}\).

If you mix olive oil with water, the olive oil will float on top of the water. The density of water is \(1.00 \mathrm{~g} / \mathrm{cm}^{3}\) at room temperature. (a) Is the density of olive oil more or less than \(1.00 \mathrm{~g} / \mathrm{cm}^{3} ?\) (b) The density of olive oil in its liquid phase does vary with temperature. Do you think olive oil would be more dense or less dense at higher temperatures? Explain.
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