Calcium oxide, CaO, is manufactured by decomposition of calcium carbonate, CaC03

Question

Calcium oxide, CaO, is manufactured by decomposition of calcium carbonate, CaC03, in a furnace: CaC03(s) rightarrow CaO(s) + C02(g) The heat produced by a furnace maintained at a temperature of 500 K can decompose calcium carbonate to calcium oxide. The spontaneity of a reaction can be determined from the free energy change for the reaction, Delta G degree. A reaction is spontaneous when the free energy change is less than zero. A reaction is nonspontaneous when the free energy change is greater than zero. A reaction is in equilibrium when the free energy change is equal to zero. Delta G degree = -RT ln K where T is the Kelvin temperature and R is equal to 8. 314 J/(mol. K). Calculate the equilibrium constant for the following reaction at room temperature, 25 degree C:CaCO3(s) rightarrow CaO(s) + CO2(g) Express your answer numerically to three significant figures. k =

Explanation / Answer

we have for this reaction

H = 178.5 KJ/mol = 178500 J/mol

S = 161 J/mol.K

T = 298.15 K

so,

G = H-TS = 130.49785 KJ/mol

equate this to -RTln(k) and solve

ln(k) = -52.6452

so,

k = 1.37x10-23 .... (in 3 significant figures)

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