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 550. L and heated to 910.0 °C. When the amount of CaCO3 has stopped changing, it is found that 567. g have disappeared. Calculate the pressure equilibrium constant K, this experiment suggests for the equilibrium between CaCO3 and CaO at 910.0 °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 K, does not match the accepted value. K-0 P X
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 550. L and heated to 910.0 °C. When the amount of CaCO3 has stopped changing, it is found that 567. g have disappeared. Calculate the pressure equilibrium constant K, this experiment suggests for the equilibrium between CaCO3 and CaO at 910.0 °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 K, does not match the accepted value. K-0 P X
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
Question
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
limestone.
Suppose some calcium carbonate is sealed into a limekiln of volume 550. L and heated to 910.0 °C. When the amount of CaCO3 has stopped changing, it is
found that 567. g have disappeared.
P
Calculate the pressure equilibrium constant K, this experiment suggests for the equilibrium between CaCO3 and CaO at 910.0 °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 K does not match the accepted value.
K-0
P
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