At 873 K, the equilibrium constant for the reaction 2PH3 (g) ⇄ P2 (g) + 3H2 (g)                      is Kp = 398. If the partial pressures of PH3 and P2 at equilibrium are 0.28 Atm and 0.71 Atm, what is the H2 concentration in moles/L?

The equilibrium constant is 1.48 for the reaction below at 800.0 K. What would be the equilibrium constant with respect to pressure, Kp, at this temperature? 2 NO2 (g) دام 2 NO (g) + O2 (g)

A mixture of 3 moles of NO and 4 moles of H2O is placed in a 5 L container and heated to 300 degrees C where the equilibrium 4NH3 (g) + 5O2 (g) ⇄ 4NO(g) + 6H2O(g) is established. At equilibrium, the NH3 , O2 , NO and H2O concentrations were 0.45, 0.5625, 0.15, and 0.125 moles/L, respectively. The volume of the container is then reduced from 5 L to 1 L. What is the equilibrium constant, Kc, after equilibrium is re-established at the reduced volume? a) 6.43x10-9 b) 1.20x106 c) 7.62x10-5 d) 3.94x108 e) 8.36x10-7

Consider the equilibrium system described by the chemical reaction below. If the partial pressures at equilibrium of NO, Cl2, and NOCI are 0.095 atm, 0.171 atm, and 0.28 atm, respectively, in a reaction vessel of 7.00 L at 500 K, what is the value of Kp for this reaction? 2 NO(g) + Cl2(g) = 2 NOCI(g)