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Calculate the values of Kp and K at 525°C with the equilibrium pressure of CO2 at 0.220 atm for the following reaction. CaCO3 (s) - CaO (s) + CO2 (g)

Calculate the values of Kp and K at 525°C with the equilibrium pressure of CO2 at 0.220 atm for the following reaction. CaCO3 (s) - CaO (s) + CO2 (g)

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
Chapter17: Spontaneity, Entropy, And Free Energy
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Calculate the values of Kp and K at 525°C with the equilibrium pressure of CO2 at 0.220
atm for the following reaction.
CaCO3 (s) - CaO (s) + CO2 (g)

SO2 (g) + NO2 (g) = SO3 (g) + NO (g) Calculate the value of Kp at the same temperature. 9. Calculate the values of Kp and Ke at 525°C with the equilibrium pressure of CO2 at 0.220 atm for the following reaction. CaCO3 (s) = CaO (s) + CO2 (g) 10. Equilibrium was established for the reaction at 2800°C from an initial pressure of HCl of 0.350 atm. 2HCI (g) = H2 (g) + Cl2 (g) The equilibrium pressure of Cl2 was 0.11 atm. What is the value of Kp for this equilibrium? 12. The dissociation of calcium carbonate has an equilibrium constant of Kp= 1.16 at 800°C. CACO3 (s) = CaO (s) + CO2 (g) What is Ke for the reaction? 233
Transcribed Image Text:SO2 (g) + NO2 (g) = SO3 (g) + NO (g) Calculate the value of Kp at the same temperature. 9. Calculate the values of Kp and Ke at 525°C with the equilibrium pressure of CO2 at 0.220 atm for the following reaction. CaCO3 (s) = CaO (s) + CO2 (g) 10. Equilibrium was established for the reaction at 2800°C from an initial pressure of HCl of 0.350 atm. 2HCI (g) = H2 (g) + Cl2 (g) The equilibrium pressure of Cl2 was 0.11 atm. What is the value of Kp for this equilibrium? 12. The dissociation of calcium carbonate has an equilibrium constant of Kp= 1.16 at 800°C. CACO3 (s) = CaO (s) + CO2 (g) What is Ke for the reaction? 233
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