At 125°C, Kp = 0.25 for the reaction 2NaHCO3(s) Na2CO3 (s) + CO2 (g) + H2O(g) A 1.00-L flask containing 39.7 g NaHCO3 is evacuated and heated to 125°C. a. Calculate the partial pressures of CO2 and H2O after equilibrium is established. Partial pressure of CO2 = Partial pressure of H2O = atm atm b. Calculate the masses of NaHCO3 and Na2CO3 present at equilibrium. Mass of NaHCO3 = Mass of Na2CO3 g g c. Calculate the minimum container volume necessary for all of the NaHCO3 to decompose. Volume = L

At 125°C, Kp = 0.25 for the reaction 2NaHCO3(s) Na2CO3 (s) + CO2 (g) + H2O(g) A 1.00-L flask containing 39.7 g NaHCO3 is evacuated and heated to 125°C. a. Calculate the partial pressures of CO2 and H2O after equilibrium is established. Partial pressure of CO2 = Partial pressure of H2O = atm atm b. Calculate the masses of NaHCO3 and Na2CO3 present at equilibrium. Mass of NaHCO3 = Mass of Na2CO3 g g c. Calculate the minimum container volume necessary for all of the NaHCO3 to decompose. Volume = L

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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