Explain why $\text{SiCl}_4$ has such a low boiling point.
$\text{SiCl}_4$ reacts with water to form an acidic solution. Write an equation for this reaction.
Describe two visual observations when silicon tetrachloride is added drop by drop to a little water.
A mass of $0.8505\,\text{g}$ of $\text{SiCl}_4$ is poured into $800\,\text{cm}^3$ of water. All of the soluble acidic product dissolves in the water. Calculate the pH of the solution formed.
Silicon tetrachloride may be made by reaction 1. reaction 1: $\text{Si(s)} + 2\text{Cl}_2(\text{g}) \rightarrow \text{SiCl}_4(\text{l}) \;\; \Delta S^\circ = -225.7\,\text{J K}^{-1}\text{mol}^{-1}$ The standard entropy of silicon is $S^\circ\,\text{Si(s)} = 18.7\,\text{J K}^{-1}\text{mol}^{-1}$. The standard entropy of silicon tetrachloride is $S^\circ\,\text{SiCl}_4(\text{l}) = 239.0\,\text{J K}^{-1}\text{mol}^{-1}$. Calculate the standard entropy of chlorine, $S^\circ\,\text{Cl}_2(\text{g})$. Show all your working.
Explain why the entropy change for reaction 1 has a negative value.
The standard enthalpy change of formation of silicon tetrachloride, $\Delta H_f^\circ\,\text{SiCl}_4(\text{l})$, is $-640\,\text{kJ mol}^{-1}$. Reaction 1 is spontaneous at lower temperatures, but becomes non-spontaneous at very high temperatures. Calculate the temperature above which reaction 1 is not spontaneous.