Question

Anastusju above. In a study of the dered Cacos) to 10 ases, then heated the cont the CO2(g) in the container CaCO3(s)--Cao(s) + CO2(g) 5. When heated, calcium carbonate decomposes according to the equation abou decomposition of calcium carbonate, a student added a 500 g sample of powd a tudy rigid container. The student sealed the container, pumped out all the gases, then in an oven at 1100 K. As the container was heated, the total pressure of the Cool was measured over time. The data are plotted in the graph below. 10 The student repeated the experiment, but this time the student used a 100.0 g sample of powdered Caco, (s). In this experiment, the final pressure in the container was 1.04 atm, which was the same final pressure as in the first experiment . Calculate the number of moles of CO2 (g) present in the container after 20 minutes of heating M . 0-HC ev n= (1004) (12) noies in 1oo84) (1100) - b. The student claimed that the final pressure in the container in each expertinent became constant because all of the caco, () had decomposed. Based on the data in the experiments, do you agree with this claim? Explain. disagree be pt constant Just bc @ equillibrium c. After 20 minutes some CO2 (g) was injected into the container, initially raising the pressure to 1.5 atm. Would the final pressure inside the container be less than, greater than or equal to 1.04 atm? Explain your reasoning stays same pressure d. Are there sufficient data obtained in the experiments to determine the value of the equilibrium constant, Kp, for the decomposition of CaCO3 (5) at 1100 R? Justify your answer. yes kp=PLO₂ = 1604

Answer 1