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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 2 limestone. Suppose some calcium carbonate is sealed into a limekiln of volume 200. L and heated to 930.0 °C. When the amount of CaCO3 has stopped changing, it is found that 1.82 kg have disappeared. Calculate the pressure equilibrium constant K. this experiment suggests for the equilibrium between CaCO3 and CaO at 930.0 °C. Round your answer to 2 significant digits. Kp Note for advanced students: it's possible there was some error in this experiment, and the value it suggests for K does not match the accepted value. P K = 0 р ☐x10 X Ś

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 2 limestone. Suppose some calcium carbonate is sealed into a limekiln of volume 200. L and heated to 930.0 °C. When the amount of CaCO3 has stopped changing, it is found that 1.82 kg have disappeared. Calculate the pressure equilibrium constant K. this experiment suggests for the equilibrium between CaCO3 and CaO at 930.0 °C. Round your answer to 2 significant digits. Kp Note for advanced students: it's possible there was some error in this experiment, and the value it suggests for K does not match the accepted value. P K = 0 р ☐x10 X Ś

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter15: Principles Of Chemical Reactivity: Equilibria
Section15.6: Disturbing A Chemical Equilibrium
Problem 1.1ACP: Anhydrous ammonia is used directly as a fertilizer, but much of it is also converted to other...
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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 2 limestone. Suppose some calcium carbonate is sealed into a limekiln of volume 200. L and heated to 930.0 °C. When the amount of CaCO3 has stopped changing, it is found that 1.82 kg have disappeared. Calculate the pressure equilibrium constant K. this experiment suggests for the equilibrium between CaCO3 and CaO at 930.0 °C. Round your answer to 2 significant digits. Kp Note for advanced students: it's possible there was some error in this experiment, and the value it suggests for K does not match the accepted value. P K = 0 р ☐x10 X Ś
Transcribed Image Text: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 2 limestone. Suppose some calcium carbonate is sealed into a limekiln of volume 200. L and heated to 930.0 °C. When the amount of CaCO3 has stopped changing, it is found that 1.82 kg have disappeared. Calculate the pressure equilibrium constant K. this experiment suggests for the equilibrium between CaCO3 and CaO at 930.0 °C. Round your answer to 2 significant digits. Kp Note for advanced students: it's possible there was some error in this experiment, and the value it suggests for K does not match the accepted value. P K = 0 р ☐x10 X Ś
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