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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 a limekiln of volume 300.L is pressurized with carbon dioxide gas to 15.5atm, and heated to 950.0°C. When the amount of CO2 has stopped changing, it is found that 1.79kg of CaCO3 have appeared. Calculate the pressure equilibrium constant Kp this experiment suggests for the equilibrium between CaCO3 and CaO at 950.0°C. Round your answer to 2 significant digits. 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.

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 CO2 from the air and turns back into hard, durable limestone.

 

Suppose a limekiln of volume 300.L is pressurized with carbon dioxide gas to 15.5atm, and heated to 950.0°C. When the amount of CO2 has stopped changing, it is found that 1.79kg of CaCO3 have appeared. Calculate the pressure equilibrium constant Kp this experiment suggests for the equilibrium between CaCO3 and CaO at 950.0°C. Round your answer to 2 significant digits.

 

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.

 

 

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