N_2(g) + 3H_2(g) 2NH_3(g) A chemist puts 6.0 moles of N_2 and 7.0 moles H_2 into an evacuated 1.0 L container. The system reaches equilibrium at a certain temperature according to the process outlined above. When the system is at equilibrium the chemist determine (NH_3) is 4.0 M. What is the equilibrium constant K_c for this process at this temperature? The diagram above represents a mixture of NO_2(g) and N_2 O_4(g) in a 1.0 L container at a given temperature. The two gases are in equilibrium according to the equation 2 NO_2(g) doubleheadarrow N_2 O_4(g) Calculate the value of the equilibrium constant for the reaction at this temperature?