Given the following equilibrium constants at 427°C:   O2(g) + 4Na(l)  2Na2O(s)     K1 = 2.50×1049   O2(g) + 2Na(l)  2NaO(g)     K2 = 2.50×109   O2(g) + 2Na(l)  Na2O2(s)     K3 = 2.00×1028   O2(g) + Na(l)  NaO2(s)     K4 = 3.33×1013 What would be the value of the equilibrium constant for each of the following reactions, at 427°C?

Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter15: Principles Of Chemical Reactivity: Equilibria
Section15.5: More About Balanced Equations And Equilibrium Constants
Problem 15.6CYU: The conversion of oxygen to ozone has a very small equilibrium constant. 3/2 O2(g) O3(g) K = 2.5 ...
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Given the following equilibrium constants at 427°C:

 

O2(g) + 4Na(l)  2Na2O(s)     K1 = 2.50×1049

 

O2(g) + 2Na(l)  2NaO(g)     K2 = 2.50×109

 

O2(g) + 2Na(l)  Na2O2(s)     K3 = 2.00×1028

 

O2(g) + Na(l)  NaO2(s)     K4 = 3.33×1013

What would be the value of the equilibrium constant for each of the following reactions, at 427°C?

 

 

Na2O2(s) + O2(g)  2NaO2(s)

 

  Incorrect. Tries 1/99 Previous Tries

 

4NaO2(s)  2Na2O(s) + 3O2(g)
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