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Chapter 10: Q70E. (page 591)
Classify each substance in the table as either a metallic, ionic, molecular, or covalent network solid
X is metallic, Y is covalent and Z is ionic solids.
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Titanium tetrachloride\(Ti{\rm{C}}{{\rm{l}}_4}\) has a melting point of\({\rm{23}}{\rm{.2}}^\circ {\rm{C}}\) and has a ΔH fusion =\(9.37\)kJ/mol.
(a) How much energy is required to melt \(263.1\)g\(Ti{\rm{C}}{{\rm{l}}_4}\)?
(b) For\(Ti{\rm{C}}{{\rm{l}}_4}\) which will likely have the larger magnitude: ΔH fusion or ΔH vaporization? Explain your reasoning.
The free space in a metal may be found by subtracting the volume of the atoms in a unit cell from the volume of the cell. Calculate the percentage of free space in each of the three cubic lattices if all atoms in each are of equal size and touch their nearest neighbours. Which of these structures represents the most efficient packing? That is, which one of them packs with the least amount of unused space?
At 20.0 °C, the vapor pressure of ethanol is 5.95 kPa, and at 63.5 °C, its vapor pressure is 53.3 kPa. Use this information to estimate the enthalpy of vaporization for ethanol.
Carbon tetrachloride, \({\rm{CC}}{{\rm{l}}_{\rm{4}}}\), was once used as a dry-cleaning solvent, but is no longer used because it is carcinogenic. At \({\bf{57}}.{\bf{8}}\)°C, the vapor pressure of \({\rm{CC}}{{\rm{l}}_{\rm{4}}}\) is \({\bf{54}}.{\bf{0}}\)kPa, and its enthalpy of vaporization is \({\bf{33}}.{\bf{05}}\)kJ/mol. Use this information to estimate the normal boiling point for \({\rm{CC}}{{\rm{l}}_{\rm{4}}}\).
Identify two common observations indicating some solids, such as dry ice and mothballs have vapour pressures sufficient to sublime.
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