Calcium oxide, CaO, is manufactured by decomposition of calcium carbonate, CaCO3
ID: 772084 • Letter: C
Question
Calcium oxide, CaO, is manufactured by decomposition of calcium carbonate, CaCO3, in a furnace: The heat produced by a furnace maintained at a temperature of 500K can decompose calcium carbonate to calcium oxide. The spontaneity of a reaction can be determined from the free energy change for the reaction, Delta . A reaction is spontaneous when the free energy change is less than zero. A reaction is nonspontaneous when the free energy is greater than zero. A reaction is in equilibrium when the free energy change is equal to zero. The thermodynamic properties for a reaction are related by the equation that defines the standard free energy, in KJ/mol: where is the standard enthalpy change in Kj/mol and is the standard entropy change in J/(mol K). A good approximation of the free energy change at other temperature, , can also be obtained by utilizing this equation and assuming enthalpy and entropy change little with temperature. For the decomposition of calcium carbonate, consider the following thermodynamic datea: Calculate the temperature in kelvins above which this reaction is spontaneous Relationship between free energy and the equilibrium constant The standard free energy change, Delta G degree, and the equilibrium constant K for a reaction can be related by the following equation: Delta G degree = - RT In 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: CaC03(s) rightarrow CaO(s) + C02(g) Express your answer numerically to three significant figures.Explanation / Answer
a) 1108 .69 K
b) 0.948
c)1.67*10^49