When magnesium carbonate is heated in a Bunsen burner flame, it decomposes. The values of the standard enthalpies of formation, $\Delta H_f^\circ$, for the species present are given below. $\Delta H_f^\circ\,\text{MgCO}_3 = -1095.8\,\text{kJ mol}^{-1}$ $\Delta H_f^\circ\,\text{MgO} = -601.7\,\text{kJ mol}^{-1}$ $\Delta H_f^\circ\,\text{CO}_2 = -393.5\,\text{kJ mol}^{-1}$ Calculate the standard enthalpy change for the decomposition of magnesium carbonate.
- A$+100.6\,\text{kJ mol}^{-1}$
- B$+887.6\,\text{kJ mol}^{-1}$
- C$+1095.8\,\text{kJ mol}^{-1}$
- D$+2091\,\text{kJ mol}^{-1}$