Magnesium chloride dissolves in water.
Table 1 shows some enthalpy data.
Table 1
| Enthalpy change | Enthalpy change / kJ mol−1\text{kJ mol}^{-1}kJ mol−1 |
|---|---|
| Enthalpy of solution of magnesium chloride | −155-155−155 |
| Enthalpy of lattice formation of magnesium chloride | −2526-2526−2526 |
| Enthalpy of hydration of magnesium ions | −1921-1921−1921 |
Use the data in Table 1 to calculate the enthalpy of hydration, in kJ mol−1\text{kJ mol}^{-1}kJ mol−1, of chloride ions.
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.