Consider the following endothermic reaction: N_2O_4(g)+Heat 2NO_2(s) (Colorless)

Question

Consider the following endothermic reaction: N_2O_4(g)+Heat 2NO_2(s) (Colorless) (Brown) In what direction would you expect the equilibrium to shift when the reaction mixture is placed in a low temperature bath? If you carried out this experiment in the lab, what change would you look for to confirm this shift? In what direction would you expect the equilibrium to shift when the reaction mixture is placed in a high temperature bath? If you carried out this experiment in the lab, what change would you look for to confirm this shift?

Explanation / Answer

a) As the reaction is endothermic, if temperature is low then backward reaction (towrdas reactants) is favourable.

b) For the above condition decrease in color change observed (brown to colorless).

c) As the reaction is endothermic, if temperature is high then forward reaction (towrdas products) is favourable.

d) For the above condition increase in color change observed (colorless to brown ).

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