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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 250. L and heated to 870.0 °C. When the amount of CaCO3 has stopped changing, it is found that 800. g have disappeared Calculate the pressure equilibrium constant Kp this experiment suggests for the equilibrium between CaCO3 and CaO at 870.0 oC. Round your answer to 2 significant digits. Note for advanced students: its possible there was some error in this experiment, and the value it suggests for Kp does not match the accepted value.

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mass af CaLos ducomposx 80o E loo Boan male a co2 CS) a- diobocia ion constanthevu e 8m molio Volume QSOL 29qa ahm p uaunon -999

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