Predict and explain how the enthalpy change of hydration varies for the ions $\text{Na}^+$, $\text{Mg}^{2+}$ and $\text{Al}^{3+}$.
Fig. 2.1 contains an incomplete energy cycle. Finish line C on Fig. 2.1. Include state symbols.
Identify change 2 on Fig. 2.1 using both words and symbols. Follow changes 1 and 3 as models for how this should be shown.
Fig. 2.1 contains an incomplete energy cycle.
Calculate a value for the lattice energy of magnesium chloride, $\Delta H_{\text{latt}}\, \text{MgCl}_2(s)$, by choosing and using suitable data from Table 2.1.
Define entropy in terms of particle arrangements and energy distribution.
At $25\,^{\circ}\text{C}$, the enthalpy change of solution for compound $Z$ is $+26\,\text{kJ mol}^{-1}$. At the same temperature, the entropy change of solution of $Z$ is $+52\,\text{J K}^{-1}\text{ mol}^{-1}$. Calculate the Gibbs free energy change, $\Delta G$, for the solution of $Z$ at $25\,^{\circ}\text{C}$.
Use your answer to (d) to predict whether or not $Z$ is soluble in water at $25\,^{\circ}\text{C}$. Explain your answer.
Predict whether $Z$ becomes more or less soluble as the water temperature rises from $25\,^{\circ}\text{C}$ to $95\,^{\circ}\text{C}$. Explain your answer.