Use the References to access Important values If needed for this question initro

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Use the References to access Important values If needed for this question initrogen tetraoxide and nitrogen dioxide are two gases that exist in equilibrium at a range of temperatures. NO2 is a reddish brown gas while N204 is col At High Temperature the red color is strong. At Low Temperature the gas has less color we represent the equilibrium as: e can conclude that: 2 NO2(g)--N204(g) 1. This reaction is: A. Exothermic B. Endothermic C. Neutral D. More information is needed to answer this question. 2. When the temperature is decreased 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 decreased the equilibrium concentration of N204 A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question.

Explanation / Answer

1.Since the product N2O4 is formed more at low temperature when less heat is available, it means the reaction doesn't require heat.So the reaction is exothermic.

Thus answer is A.

2.Equilibrium constant k= concentration of N2O4 formed/NO2 reacted.

So K increases as T decreases.

So answer is A.

3.A

Comment in case of any doubt.

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