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Dinitrogen trioxide decomposes to NO and NO2 in an endothermic process (DHo = + 40.5 kJ/mol)? N2O3 (g)   NO2 (g) + NO (g)       Predict the effect the following changes on the position of equilibrium; in other words, state which way the equilibrium will shift (left, right, no change) when each of the following changes is made. Adding more N2O3 (g) Removing NO2 (g) Adding more NO (g) Lowering the temperature Moving the system to a smaller flask

Dinitrogen trioxide decomposes to NO and NO2 in an endothermic process (DHo = + 40.5 kJ/mol)? N2O3 (g)   NO2 (g) + NO (g)       Predict the effect the following changes on the position of equilibrium; in other words, state which way the equilibrium will shift (left, right, no change) when each of the following changes is made. Adding more N2O3 (g) Removing NO2 (g) Adding more NO (g) Lowering the temperature Moving the system to a smaller flask

Introductory Chemistry: A Foundation
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 126CP: . Consider the following exothermic reaction at equilibrium: N2(g)+3H2(g)2NH3(g)Predict how the...
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  1. Dinitrogen trioxide decomposes to NO and NO2 in an endothermic process (DHo = + 40.5 kJ/mol)?

N2O3 (g)   NO2 (g) + NO (g)

     

Predict the effect the following changes on the position of equilibrium; in other words, state which way the equilibrium will shift (left, right, no change) when each of the following changes is made.

  1. Adding more N2O3 (g)

  2. Removing NO2 (g)

  3. Adding more NO (g)

  4. Lowering the temperature

  5. Moving the system to a smaller flask

 

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