Dinitrogen tetraoxide and nitrogen dioxide are two gases that exist in equilibrium at a range of temperatures. NO₂ is a reddish brown gas while N₂O4 is colorles At high temperature the red color is strong. At low temperature the gas has less color. If we represent the equilibrium as: 2 NO2 (9) N₂ 04 (9) We can conclude that: 1. This reaction is Oexothermic. O endothermic. O neutral. O More information is needed to answer this question. 2. When the temperature is decreased the equilibrium constant, K: O increases. O decreases. O remains the same. O More information is needed to answer this question. 3. When the temperature is decreased the equilibrium concentration of N₂ 04: O increases. O decreases. O remains the same. O More information is needed to answer this question.
Dinitrogen tetraoxide and nitrogen dioxide are two gases that exist in equilibrium at a range of temperatures. NO₂ is a reddish brown gas while N₂O4 is colorles At high temperature the red color is strong. At low temperature the gas has less color. If we represent the equilibrium as: 2 NO2 (9) N₂ 04 (9) We can conclude that: 1. This reaction is Oexothermic. O endothermic. O neutral. O More information is needed to answer this question. 2. When the temperature is decreased the equilibrium constant, K: O increases. O decreases. O remains the same. O More information is needed to answer this question. 3. When the temperature is decreased the equilibrium concentration of N₂ 04: O increases. O decreases. O remains the same. O More information is needed to answer this question.
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 54P
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Transcribed Image Text:Dinitrogen tetraoxide and nitrogen dioxide are two gases that exist in equilibrium at a range of temperatures. NO2 is a reddish brown gas while N₂O4 is colorless.
At high temperature the red color is strong. At low temperature the gas has less color.
If we represent the equilibrium as:
2 NO2 (g) N₂O4 (9)
We can conclude that:
1. This reaction is
exothermic.
O endothermic.
O neutral.
O More information is needed to answer this question.
2. When the temperature is decreased the equilibrium constant, K:
O increases.
O decreases.
O remains the same.
O More information is needed to answer this question.
3. When the temperature is decreased the equilibrium concentration of N₂ 04:
O increases.
O decreases.
O remains the same.
O More information is needed to answer this question.
Transcribed Image Text:Dinitrogen tetraoxide and nitrogen dioxide are two gases that exist in equilibrium at a range of temperatures. NO2 is a reddish brown gas while N₂O4 is colorless.
At high temperature the red color is strong. At low temperature the gas has less color.
If we represent the equilibrium as:
2 NO2 (9) N₂O4 (9)
We can conclude that:
1. This reaction is
Oexothermic.
O endothermic.
O neutral.
O More information is needed to answer this question.
2. When the temperature is increased the equilibrium constant, K:
O increases.
O decreases.
O remains the same.
O More information is needed to answer this question.
3. When the temperature is increased the equilibrium concentration of N₂ 04:
increases.
O decreases.
O remains the same.
O More information is needed to answer this question.
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