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.

explanation:

let the different atoms be x and y. each with four protons and same mass will be represented as follows.

mass number is number of protons + number of neutrons.

            and  

since, it is given that one has a negative charge while the other is neutral. therefore, there will be increase in number of protons and the atom will be represented as follows.

according to periodic table, mass number of beryllium is 9 and it has atomic number 4 so, the atoms will be and .  

the protons and neutrons will be located inside the nucleus whereas the electrons will be revolving around the nucleus.