A mixture of NO3 and a ten-fold excess of NO2 are placed inside a rigid container at constant temperature and allowed to reach equilibrium. Which of the following provides a correct comparison of the equilibrium concentrations of these chemical species, and why?

[N₂O₅]<<[NO₂] because a small K value indicate that the formation of the is not favoured at equilibrium.

Explanation:

* the question appear to be incomplete, as the first part of it is missing out

At night an equilibrium reaction between two different nitrogen compounds generates N2O5 in the atmosphere as represented below

NO3(g) + NO2(g) <> N2O5(g)

K=2.6x10^-11

Options:

a.) |N2O5|<<|NO3| because a small value of K indicates that the consumption of reactants is favored at equilibrium.

b.)  |NO2|<<|N2O5| because a small value of K indicates that the consumption of reactants is favored at equilibrium.

c.) |NO2|<<|NO3| because a small value of K indicates that the formation of products is not favored at equilibrium.

d.) |N2O5| << |NO2| because a small value of K indicates that the formation of products is not favored at equilibrium.

c, liquids evaporate, creating a gas