Sodium hydrogen carbonate decomposes above 110 °C to form sodium carbonate, water, and carbon dioxide. 2NaHCO3(s) ↔ Na2CO3(s) + H2O(g) + CO2(g) One thousand grams of sodium hydrogen carbonate are added to a reaction vessel, the temperature is increased to 200 °C, and the system comes to equilibrium. What happens to the partial pressure of carbon dioxide in this system if 50 g of sodium carbonate are added?
Sodium hydrogen carbonate decomposes above 110 °C to form sodium carbonate, water, and carbon dioxide. 2NaHCO3(s) ↔ Na2CO3(s) + H2O(g) + CO2(g) One thousand grams of sodium hydrogen carbonate are added to a reaction vessel, the temperature is increased to 200 °C, and the system comes to equilibrium. What happens to the partial pressure of carbon dioxide in this system if 50 g of sodium carbonate are added?
Introductory Chemistry: A Foundation
9th Edition
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Donald J. DeCoste
Chapter17: Equilibrium
Section: Chapter Questions
Problem 12ALQ: In Section 17.3 of your text, it is mentioned that equilibrium is reached in a closed system. What...
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- Sodium hydrogen carbonate decomposes above 110 °C to form sodium carbonate, water, and carbon dioxide.
2NaHCO3(s) ↔ Na2CO3(s) + H2O(g) + CO2(g)
One thousand grams of sodium hydrogen carbonate are added to a reaction vessel, the temperature is increased to 200 °C, and the system comes to equilibrium. What happens to the partial pressure of carbon dioxide in this system if 50 g of sodium carbonate are added?
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