Example Problem For the reaction, N2 (g) + 3H2 (g) , the equilibrium constant Kp = 1.45 X10-5 at 500 degrees Celsius. In an equilibrium mixture of the three gases, the partial pressure of H2 is 0.928 atm and that of N2 is 0.432 atm. A) Calculate the partial pressure of NH3 in the mixture. I came up with 2.24 * 10^-3 atm. B) Calculate the equilibrium constant Kc at 500 degrees Celsius. I'm not sure is it 1.45*10^-5? I need help w/ this part. C) Calculate the equilibrium constant Kp for the reaction NH3 (g) 1/2 N2 (g) + 3/2 H2 (g).

Question

Example Problem For the reaction, N2 (g) + 3H2 (g) <=>, the equilibrium constant Kp = 1.45 X10-5 at 500 degrees Celsius. In an equilibrium mixture of the three gases, the partial pressure of H2 is 0.928 atm and that of N2 is 0.432 atm. A) Calculate the partial pressure of NH3 in the mixture. I came up with 2.24 * 10^-3 atm. B) Calculate the equilibrium constant Kc at 500 degrees Celsius. I'm not sure is it 1.45*10^-5? I need help w/ this part. C) Calculate the equilibrium constant Kp for the reaction NH3 (g) <=> 1/2 N2 (g) + 3/2 H2 (g).