The equilibrium established in N2O (g) <---> 2NO2 (g) is a common example in che

Question

The equilibrium established in N2O (g) <---> 2NO2 (g) is a common example in chemistry texts since NO2 is brown while N2O is light yellow. This means the equilibrium can be followed via color. Delta H for this reaction can be calculated as 58.04 kJ/mol rxn. A). What happens to the position of the equilibrium if the reaction vessel is placed in a boiling water bath? B). What happens to the position of the equilibrium if the volume of the reaction vessel is decreased? C). How would these changes appear as to color?

Explanation / Answer

A. The reaction will proceed in forward direction because reaction is endothermic and it favours increased temperature. B. The reaction is N2O 2NO2, so delta ng = 2-1 =1 Since no of moles is decreased in reverse direction, hence decreasing the volume will favour the reaction to move in reverse direction. C. In case A the colour appears to be brownish whereas in case B it will be more yellowish

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