The equilibrium constant Kₚ for the reaction 2 NO₂(g) ⇌ N₂O₄(g) is 0.50 at 298 K
CHEMISTRY · Single correct · AP · Chemistry · Equilibrium · Equilibrium
Problem
The equilibrium constant Kₚ for the reaction 2 NO₂(g) ⇌ N₂O₄(g) is 0.50 at 298 K. A sealed flask at 298 K contains partial pressures P(NO₂) = 0.60 atm and P(N₂O₄) = 0.10 atm. What will happen as the mixture moves toward equilibrium at 298 K?
(a) The reverse reaction is favored because Q>K, so N2O4 will dissociate.
(b) The forward reaction is favored because Q<K, so NO2 will be consumed.
(c) The system is already at equilibrium because Q=K, so no net change occurs.
(d) The forward reaction is favored because Q>K, so NO2 will be consumed.