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Calcium carbonate, CaCO3, decomposes when heated to give calcium oxide, CaO, and carbon dioxide, CO₂. CaCO3(s) CaO(s) + CO₂(g) Kp for this reaction at 940.°C is 1.216. a. What would be the yield of carbon dioxide (in grams) when 8.218 g of CaCO3 and 8.218 g CaO are heated to 940.°C in a 8.400 L vessel. (Ignore the volume occupied by the solids.) Mass of CO2 g b. What would be the masses at equilibrium if the quantity of CO2 obtained in part a were doubled? Mass of CO₂ = g Mass of CaO = g Mass of CaCO3 = g c. What would be the masses at equilibrium if the quantity of calcium carbonate in part a were doubled?

Calcium carbonate, CaCO3, decomposes when heated to give calcium oxide, CaO, and carbon dioxide, CO₂. CaCO3(s) CaO(s) + CO₂(g) Kp for this reaction at 940.°C is 1.216. a. What would be the yield of carbon dioxide (in grams) when 8.218 g of CaCO3 and 8.218 g CaO are heated to 940.°C in a 8.400 L vessel. (Ignore the volume occupied by the solids.) Mass of CO2 g b. What would be the masses at equilibrium if the quantity of CO2 obtained in part a were doubled? Mass of CO₂ = g Mass of CaO = g Mass of CaCO3 = g c. What would be the masses at equilibrium if the quantity of calcium carbonate in part a were doubled?

Chemistry
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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Calcium carbonate, CaCO3, decomposes when heated to give calcium oxide, CaO, and carbon dioxide, CO₂. CaCO3(s) CaO(s) + CO₂(g) Kp for this reaction at 940.°C is 1.216. a. What would be the yield of carbon dioxide (in grams) when 8.218 g of CaCO3 and 8.218 g CaO are heated to 940.°C in a 8.400 L vessel. (Ignore the volume occupied by the solids.) Mass of CO2 g = b. What would be the masses at equilibrium if the quantity of CO2 obtained in part a were doubled? Mass of CO₂ = g Mass of CaO = Mass of CaCO3 = g c. What would be the masses at equilibrium if the quantity of calcium carbonate in part a were doubled? Mass of CO2 = g Mass of CaO = Mass of CaCO3 g = g
Transcribed Image Text:Calcium carbonate, CaCO3, decomposes when heated to give calcium oxide, CaO, and carbon dioxide, CO₂. CaCO3(s) CaO(s) + CO₂(g) Kp for this reaction at 940.°C is 1.216. a. What would be the yield of carbon dioxide (in grams) when 8.218 g of CaCO3 and 8.218 g CaO are heated to 940.°C in a 8.400 L vessel. (Ignore the volume occupied by the solids.) Mass of CO2 g = b. What would be the masses at equilibrium if the quantity of CO2 obtained in part a were doubled? Mass of CO₂ = g Mass of CaO = Mass of CaCO3 = g c. What would be the masses at equilibrium if the quantity of calcium carbonate in part a were doubled? Mass of CO2 = g Mass of CaO = Mass of CaCO3 g = g
The following equilibrium was studied by analyzing the equilibrium mixture for the amount of HCl produced. LaCl3 (s) + H₂O(g) ⇒ LaOCl(s) + 2HCl(g) A vessel whose volume was 6.15 L was filled with 1.40 × 10-2 mol of lanthanum(III) chloride, LaCl3, and 2.80×10-² mol H₂O. After the mixture came to equilibrium in the closed vessel at 619°C, the gaseous mixture was removed and dissolved in more water. Sufficient silver ion was added to precipitate the chloride ion completely as silver chloride. If 4.01 g AgCl was obtained, what is the value of Ke at 619°C? Kc =
Transcribed Image Text:The following equilibrium was studied by analyzing the equilibrium mixture for the amount of HCl produced. LaCl3 (s) + H₂O(g) ⇒ LaOCl(s) + 2HCl(g) A vessel whose volume was 6.15 L was filled with 1.40 × 10-2 mol of lanthanum(III) chloride, LaCl3, and 2.80×10-² mol H₂O. After the mixture came to equilibrium in the closed vessel at 619°C, the gaseous mixture was removed and dissolved in more water. Sufficient silver ion was added to precipitate the chloride ion completely as silver chloride. If 4.01 g AgCl was obtained, what is the value of Ke at 619°C? Kc =
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