Anhydrous calcium bromide, CaBr2\text{CaBr}_2CaBr2, dissolves readily in water to form an aqueous solution.
Table 1 shows some thermodynamic enthalpy data associated with this process.
Table 1
| Enthalpy change | Enthalpy change / kJ mol−1\text{kJ mol}^{-1}kJ mol−1 |
|---|---|
| Enthalpy of solution of calcium bromide | −144-144−144 |
| Enthalpy of lattice formation of calcium bromide | −2176-2176−2176 |
| Enthalpy of hydration of calcium ions | −1650-1650−1650 |
Use the data in Table 1 to calculate the enthalpy of hydration, in kJ mol−1\text{kJ mol}^{-1}kJ mol−1, of bromide 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.