Calcium carbonate decomposes in a lime kiln according to CaCO_3(s) ; ; CaO(s)+CO_2(g)…

CHEMISTRY · Multi-part · CBSE · Chemistry · Thermodynamics · Thermodynamics

Problem

Calcium carbonate decomposes in a lime kiln according to

\mathrm{CaCO_3(s)\;\longrightarrow\; CaO(s)+CO_2(g)}

with an enthalpy change of

\Delta H=+178\,\text{kJ\,mol}^{-1}

. An industrial facility needs to absorb

1.20\times10^{10}\,\text{J}

of thermal energy for a high-temperature process, and the only available source of heat absorption is the decomposition of calcium carbonate. In practice, the kiln operates at

88\%

yield: only

88\%

of the calcium carbonate that is fed into the kiln actually decomposes. (a) Determine the number of moles of

\mathrm{CaCO_3}

that must decompose (i.e., actually undergo reaction) to absorb the required thermal energy. (b) Calculate the mass of

\mathrm{CaCO_3}

, in kilograms, that must decompose to supply this energy. (c) Taking the

88\%

yield into account, calculate the minimum mass of solid

\mathrm{CaCO_3}

that must be loaded into the kiln. (d) Identify one operational factor that could cause the decomposition yield to deviate from the ideal

88\%

, and briefly explain its effect.

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