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 CO₂ from the air and turns back into hard, durable limestone Suppose some calcium carbonate is sealed into a limekiln of volume 600. L and heated to 520.0 °C. When the amount of CaCO₃ has stopped changing, it is found that 8.3 kg have disappeared. Calculate the pressure equilibrium constant, this experiment suggests for the equilibrium between CaCO₃ and CaO at 520.0°C.
