The reaction [2 NO2 (g) -- N204(g)] has an equilibrium constant Kc=170 at 25 deg C. If 2.0x10^-3 mol of NO2 is present in a 10.0 L flask along with 1.5x10^-3 mol of N204, is the system at equilibrium? If it is not an equilibrium, does the concentration of NO2 increase or decrease as the system proceeds?

Question

The reaction [2 NO2 (g) --> N204(g)] has an equilibrium constant Kc=170 at 25 deg C. If 2.0x10^-3 mol of NO2 is present in a 10.0 L flask along with 1.5x10^-3 mol of N204, is the system at equilibrium? If it is not an equilibrium, does the concentration of NO2 increase or decrease as the system proceeds?

anonymous · Answer

WOuld it decrease because NO2 is larger?