The decomposition of limestone, CaCO3(s), into quicklime,...

The decomposition of limestone, $\mathrm{CaCO}_{3}(\mathrm{s}),$ into quicklime, $\mathrm{CaO}(\mathrm{s}),$ and $\mathrm{CO}_{2}(\mathrm{g})$ is carried out in a gas-fired kiln. Use data from Appendix D to determine how much heat is required to decompose $1.35 \times 10^{3} \mathrm{kg} \mathrm{CaCO}_{3}(\mathrm{s}) .$ (Assume that heats of reac- tion are the same as at $25^{\circ} \mathrm{C}$ and 1 bar.)

The decomposition of limestone, $\mathrm{CaCO}_{3}(\mathrm{s}),$ into quicklime, $\mathrm{CaO}(\mathrm{s}),$ and $\mathrm{CO}_{2}(\mathrm{g})$ is carried out in a gas-fired kiln. Use data from Appendix D to determine how much heat is required to decompose $1.35 \times 10^{3} \mathrm{kg} \mathrm{CaCO}_{3}(\mathrm{s}) .$ (Assume that heats of reac-
tion are the same as at $25^{\circ} \mathrm{C}$ and 1 bar.)

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Key Concepts

Chemical Stoichiometry

Stoichiometry involves the quantitative relationships between reactants and products in a balanced chemical reaction. It allows the conversion of quantities (such as mass) of reactants into the corresponding amounts (in moles) required or produced in the reaction, laying the groundwork for accurately calculating energy changes.

Mass-to-Mole Conversion

This concept involves converting the mass of a substance to the number of moles using its molar mass. It is a fundamental step in applying stoichiometric relationships to chemical reactions, as thermodynamic data—such as enthalpy changes—are typically given per mole of substance, making the conversion essential for energy calculations.

Enthalpy of Reaction

This concept refers to the heat absorbed or released during a chemical reaction at constant pressure. It is often expressed in kilojoules per mole and enables one to calculate the overall energy change of a reaction, which is essential for determining the heat required or produced during a chemical transformation.

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