In which of the following reactions would increasing pressure at constant temperature not change the...?

Question

In which of the following reactions would increasing pressure at constant temperature not change the concentrations of the reactants and products, based on Le Chateliers principle? Please explain thank you so much! :)

A.) N2O4 <---> 2(NO2)

B.) 2(N2) + O2<-->2(N2O)

C.) N2 + 3(H2) <--> 2 (NH3)

D.) N2 + 2(O2) <-->2(NO2)

E.) N2 + O2 <--> 2NO

E

Answer 1

A change in pressure will change the equilibrium in all cases where there is a difference in moles (and hence volumes) of reactants and products.

A) 1:2 will change

B) 3:2 will change

C) 4:2 Will change

D) 3:2 will change

E) 2:2 Will not chage.

E is the only answer.

Answer 2

  you are right , it is             E.) N2 + O2 &lt;--&gt; 2NO

whenever the # of moles of gases of products = the # of moles of gases of reactants,... changing the pressure has no effect