Chapter 15, Problem 98E

When N₂O₅(g) is heated, it dissociates into N₂O₃(g) and O₂(g) according to the reaction:

${\text{N}}_{\text{2}}{\text{O}}_{\text{5}}\left(\text{g}\right)\rightleftharpoons {\text{N}}_{\text{2}}{\text{O}}_{\text{3}}\left(\text{g}\right)+{\text{O}}_{\text{2}}\left(\text{g}\right)$K_c= 7.75 at a given temperature

The N₂O₃(g) dissociates to give N₂O₃(g) and O₂(g) to the reaction:

${\text{N}}_{\text{2}}{\text{O}}_3\left(\text{g}\right)\rightleftharpoons {\text{N}}_{\text{2}}\text{O}\left(\text{g}\right)+{\text{O}}_{\text{2}}\left(\text{g}\right)$K_c= 4.00 at a given temperature
When 4.00 moI of N₂O₅(g) is heated in a 1.00-L reaction vessel to this temperature, the concentration of O₂(g) at equilibrium is 4.50 moL/L. Find the concentrations of all the other species in the equilibrium system.