Write an equation, including state symbols, to represent the process that occurs when the enthalpy of solution of strontium chloride, SrCl2\text{SrCl}_2SrCl2, is measured.
Table 1 shows some thermodynamic data.
Table 1
| Process / Quantity | Enthalpy change / kJ mol−1\text{kJ mol}^{-1}kJ mol−1 |
|---|---|
| Enthalpy of lattice dissociation of SrCl2\text{SrCl}_2SrCl2 | +2150+2150+2150 |
| Enthalpy of hydration of Sr2+(g)\text{Sr}^{2+}(g)Sr2+(g) | −1445-1445−1445 |
| Enthalpy of hydration of Cl−(g)\text{Cl}^-(g)Cl−(g) | −363-363−363 |
Use the data in Table 1 to calculate the value for the enthalpy of solution of strontium chloride.
The enthalpy of hydration of Be2+(g)\text{Be}^{2+}(g)Be2+(g) is −2494 kJ mol−1-2494\text{ kJ mol}^{-1}−2494 kJ mol−1.
Suggest why the enthalpy of hydration for Be2+(g)\text{Be}^{2+}(g)Be2+(g) is significantly more exothermic than that of Sr2+(g)\text{Sr}^{2+}(g)Sr2+(g).
27 exam-style questions on AQA A Level Chemistry Thermodynamics (A-level only), covering Born–Haber cycles (A-level only) and Gibbs free-energy change, $\Delta G$ , and entropy change, $\Delta S$ (A-level only). Each one has a worked solution and a mark scheme showing where the marks go.