At 125°C, Kp = 0.25 for the reaction 2NaHCO3(s) = Na2CO3(s) + CO2(9) + H2O(g) A 1.00-L flask containing 15.1 g NaHCO3 is evacuated and heated to 125°C. a. Calculate the partial pressures of CO2 and H20 after equilibrium is established. Partial pressure of CO2 = 0.5 atm Partial pressure of H20 = 0.5 atm b. Calculate the masses of NaHCO3 and Naz CO3 present at equilibrium. Mass of NaHCO3 %3D Mass of Naz CO3 = c. Calculate the minimum container volume necessary for all of the NaHCO3 to decompose Volume =

At 125°C, Kp = 0.25 for the reaction 2NaHCO3(s) = Na2CO3(s) + CO2(9) + H2O(g) A 1.00-L flask containing 15.1 g NaHCO3 is evacuated and heated to 125°C. a. Calculate the partial pressures of CO2 and H20 after equilibrium is established. Partial pressure of CO2 = 0.5 atm Partial pressure of H20 = 0.5 atm b. Calculate the masses of NaHCO3 and Naz CO3 present at equilibrium. Mass of NaHCO3 %3D Mass of Naz CO3 = c. Calculate the minimum container volume necessary for all of the NaHCO3 to decompose Volume =

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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