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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Question
![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](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3e1c88b1-11f2-4a05-b0dc-2aada90fd1ae%2Fecd4ba21-a1c7-4173-b666-02aec211010e%2Fmhz3gbl_processed.png&w=3840&q=75)
Transcribed Image Text: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
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