When heated calcium carbonate decomposes according to the equation below. CaCO3(s) → CO2(g) + CaO (s) In a study of the decomposition of calcium carbonate, a student added a 25.0 g sample of powdered CaCO3(s) into a rigid 2.0 L container. The student sealed the container, pumped out all the gases, then heated the container in an oven at 1100 K. As the container was heated, the total pressure of the CO2in the container was measured over time. The data are plotted in the graph below. The student repeated the experiment but this time the student used a 50 g sample of powdered CaCO3(s). In this experiment, the final pressure in the container was 1.04 atm, which is the same final pressure as in the first experiment. f. The student claimed the final pressure in the container and each experiment became constant because all of the CaCO3 had decomposed. Based on the data in the experiments do you agree with this claim? Explain.
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
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.
When heated calcium carbonate decomposes according to the equation below. CaCO3(s) → CO2(g) + CaO (s)
In a study of the decomposition of calcium carbonate, a student added a 25.0 g sample of powdered CaCO3(s) into a rigid 2.0 L container. The student sealed the container, pumped out all the gases, then heated the container in an oven at 1100 K. As the container was heated, the total pressure of the CO2in the container was measured over time. The data are plotted in the graph below.
The student repeated the experiment but this time the student used a 50 g sample of powdered CaCO3(s). In this experiment, the final pressure in the container was 1.04 atm, which is the same final pressure as in the first experiment.
f. The student claimed the final pressure in the container and each experiment became constant because all of the CaCO3 had decomposed. Based on the data in the experiments do you agree with this claim? Explain.
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