Define entropy in terms of disorder.
Predict the sign of the standard entropy change for reaction 1. Explain your reasoning.
Use the data in Table 3.1 to demonstrate that the enthalpy change for the reaction below is $-196\,\text{kJ mol}^{-1}$. $\text{2H}_2\text{O}_2(g) \rightarrow \text{2H}_2\text{O}(g) + \text{O}_2(g)$
The enthalpy change and Gibbs free energy change for the reaction below are given. $\text{2H}_2\text{O}_2(l) \rightarrow \text{2H}_2\text{O}(l) + \text{O}_2(g)$ $\Delta H^\circ = -196\,\text{kJ mol}^{-1}$ $\Delta G^\circ = -238\,\text{kJ mol}^{-1}$ Several standard entropies, $S^\circ$, are listed. Use the information provided to calculate the standard entropy of oxygen, $S^\circ$, $\text{O}_2(g)$.
The decomposition of $\text{H}_2\text{O}_2(aq)$ is catalysed by aqueous iron(III) chloride and by silver metal. Identify which catalyst is homogeneous. Explain your answer.
An electrochemical cell is set up with these half-cells: an acidified $\text{H}_2\text{O}_2$ solution with a platinum wire, and $\text{Cr}^{2+}$ mixed with $\text{Cr}^{3+}$ with a platinum wire. Identify the positive half-cell and work out the standard cell potential, $E^{\circ}_{\text{cell}}$.
Calculate $\Delta G^{\circ}$ for the cell reaction that takes place, per mole of $\text{H}_2\text{O}_2$.
Use the Nernst equation to determine $E$, the electrode potential of half-cell 2 under these conditions.
Write an equation for the cell reaction occurring in this cell under these conditions.
Define the enthalpy change of hydration, $\Delta H_{\text{hyd}}$.
Aluminium fluoride, $\text{AlF}_3$, is an ionic solid. Complete and annotate the energy cycle to show how the enthalpy change of solution of $\text{AlF}_3$, $\Delta H^{\circ}_{\text{sol}}$, is related to the lattice energy of $\text{AlF}_3$, $\Delta H^{\circ}_{\text{latt}}$, and the enthalpy changes of hydration of $\text{Al}^{3+}$ and $\text{F}^-$, $\Delta H^{\circ}_{\text{hyd}}$. Include state symbols for all ions and substances.
Use the given data and the energy cycle in (g)(ii) to calculate the lattice energy, $\Delta H^{\circ}_{\text{latt}}$, of $\text{AlF}_3$.