Calcium carbonate decomposes in industrial lime kilns according to the balanced…

CHEMISTRY · Multi-part · A Level · Chemistry · Energetics · Energetics

Problem

Calcium carbonate decomposes in industrial lime kilns according to the balanced equation CaCO3(s)→CaO(s)+CO2(g)ΔHrxn∘=?\mathrm{CaCO_3}(s) \rightarrow \mathrm{CaO}(s) + \mathrm{CO_2}(g) \quad \Delta H^\circ_{\mathrm{rxn}} = ? The following standard molar enthalpies of formation are available at 298 K: CaCO3(s): −1207 kJ mol−1\mathrm{CaCO_3}(s):\ -1207\,\text{kJ}\,\text{mol}^{-1} CaO(s): −635.5 kJ mol−1\mathrm{CaO}(s):\ -635.5\,\text{kJ}\,\text{mol}^{-1} CO2(g): −393.5 kJ mol−1\mathrm{CO_2}(g):\ -393.5\,\text{kJ}\,\text{mol}^{-1} The molar mass of CaCO3\mathrm{CaCO_3} is 100.1 g mol−1100.1\,\text{g}\,\text{mol}^{-1}. (a) Calculate the standard enthalpy change, ΔHrxn∘\Delta H^\circ_{\mathrm{rxn}}, for the decomposition of 1.001.00 mol of CaCO3\mathrm{CaCO_3} at 298 K298\,\text{K}. (b) State whether the decomposition is endothermic or exothermic and justify your answer with reference to the numerical result from part (a). (c) A kiln processes 5.05.0 metric tons of CaCO3\mathrm{CaCO_3} per day. Estimate the quantity of heat (in megajoules) that must be supplied or removed each day to carry out the decomposition under standard conditions, based on the value obtained in part (a).

Related theory

Browse the problem library