Question

When limestone (solid CaCO3) is heated, it decomposes into lime (solid CaO) and carbon dioxide gas. This is an extremely useful industrial process of great antiquity, because powdered lime mixed with water is the basis for mortar and concrete the lime absorbs CO, from the air and turns back into hard, durable limestone Suppose a limekiln of volume 350. L is pressurized with carbon dioxide gas to 5.60 atm, and heated to 1110. °C. When the amount of CO2 has stopped changing, it is found that 617. g of CaCO3 have appeared alo Calculate the pressure equilibrium constant K, this experiment suggests for the equilibrium between CaCO3 and CaO at 1110. °C. Round your answer to 2 significant digits Ar Note for advanced students: it's possible there was some error in this experiment, and the value it suggests for Kp does not match the accepted value. x 10

Answer 1

The following reaction is occurring: CaCO_3 (s) rightarrow CaO (s) + CO_2 (g) The equilibrium constant of the given equation is as follows: K_p = p_CO_2 All the other component except CO_2 are in solid state, thus, only CO_2 (g) will be considered for the equilibrium constant (K_p) The mass of calcium carbonate appeared is given as 6.95 Kg = 6950 g. Determine the moles of calcium carbonate appeared as shown below: Moles = Given mass of CaCO_3/Molecular mass of CaCO_3 = 6950 g/100 g/mol = 69.5 mol From the equation, 1 mole of CaCO_3 gives 1 mole of CO_2 (g): thus, 69.5 moles of CaCO_3 gives 69.5 moles of CO_2 (g). The pressure of CO_2 (g) is given as 14.9 atm. The volume of CO_2 (g) is given as 850 L. The temperature is given as 920 degree C = 1193.15 K. Determine the moles of CO_2 (g) present initially using ideal gas equation as shown below: PV = nRT n = PV/RT

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