When limestone (solid CaCO3) is heated, it decomposes into lime (solid CaO) and carbon dioxide gas. This

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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 750.L and heated to 770.0°C

When the amount of CaCO3 has stopped changing, it is found that 8.77kg have disappeared.

Calculate the pressure equilibrium constant Kp this experiment suggests for the equilibrium between CaCO3 and CaO at 770.0°C Round your answer to 2 significant digits.

Posted Date: Nov 17, 2021 05:15 AM

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When limestone (solid CaCO3) is heated, it decomposes into lime (solid CaO) and carbon dioxide gas. This

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Given T 7700 C 7700 2731s K T043 IS K V 750 L Now from chem... View the full answer

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