🤓 Based on our data, we think this question is relevant for Professor Todd's class at VANDERBILT.
N2O5(g) ⇌ N2O3(g) + O2(g); Kc = 7.75
[N2O5] = 4.00 M
x = 2.5306
x = [N2O3]
[N2O3] = 2.5306 M
N2O3(g) ⇌ N2O(g) + O2(g); Kc = 4.00
When N2O5(g) is heated it dissociates into N2O3(g) and O2(g) according to the following reaction:
N2O5(g) ⇌ N2O3(g) + O2(g); Kc = 7.75 at a given temperature
The N2O3(g) dissociates to give N2O(g) and O2(g) according the following reaction:
N2O3(g) ⇌ N2O(g) + O2(g); Kc = 4.00 at the same temperature
When 4.00 mol 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 concentration of N2O3 in the equilibrium system.