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Dinitrogen tetraoxide and nitrogen dioxide are two gases that exist in equilibrium at a range of...

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(g) We can conclude that: 1. This reaction is: A. Exothermic B. Endothermic C. Neutral D. More information is needed to answer this question. 2. When the temperature is increased the equilibrium constant, K: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question. 3. When the temperature is increased the equilibrium concentration of NO2: A. Increases

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Answer #1

Formation of N2O4 is an exothermic reaction, therefore, decreasing the temperature will shift the equilibrium in favour of colourless N2O4. Similarly, the formation of NO2 is an endothermic reaction, increasing the temperature will shift the equilibrium in favour of NO2

2NO2(g)   N2O4(g)

1) This reaction is:

Answer: A. Exothermic

2) When the temperature is increased the equilibrium constant, K

If the forward reaction is exothermic, then increasing the temperature will decrease the equilibrium constant

Answer: B. Decreases

3) When the temperature is increased the equilibrium concentration of NO2:

Increasing the temperature will favour the endothermic process

Answer: Increases

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