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1.1 1 (a) N₂(g) = + 180 kJ mol-¹ + O₂(g) (b) Increasing the pressure From the equilibrium shown above, use Le Chatelier's Principle to decide what happens to the equilibrium position by: (a) Increasing the concentration of NO (c) Increasing the temperature (d) Increasing the concentration of N₂ (e) Adding a catalyst 2NO (g) AH 298

1.1 1 (a) N₂(g) = + 180 kJ mol-¹ + O₂(g) (b) Increasing the pressure From the equilibrium shown above, use Le Chatelier's Principle to decide what happens to the equilibrium position by: (a) Increasing the concentration of NO (c) Increasing the temperature (d) Increasing the concentration of N₂ (e) Adding a catalyst 2NO (g) AH 298

Chemistry
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter13: Chemical Equilibrium
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Problem 11ALQ: Explain why the development of a vapor pressure above a liquid in a closed container represents an...
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1.1 1 (a) N₂(g) = + 180 kJ mol-¹ + O₂(g) (b) Increasing the pressure From the equilibrium shown above, use Le Chatelier's Principle to decide what happens to the equilibrium position by: (a) Increasing the concentration of NO (c) Increasing the temperature (d) Increasing the concentration of N₂ (e) Adding a catalyst 2NO (g) ΔΗ, 298
Transcribed Image Text:1.1 1 (a) N₂(g) = + 180 kJ mol-¹ + O₂(g) (b) Increasing the pressure From the equilibrium shown above, use Le Chatelier's Principle to decide what happens to the equilibrium position by: (a) Increasing the concentration of NO (c) Increasing the temperature (d) Increasing the concentration of N₂ (e) Adding a catalyst 2NO (g) ΔΗ, 298
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