For the synthesis of ammonia from H2(g) and N2(g) by the reaction below, K = 6.2x105 at 298 K and K = 9.06x10-2 at 500 K. 3H2(g) + N2(g) 2NH3(g) The reaction is exothermic by 92.22 kJ/mole. Suppose that hydrogen and nitrogen are reacted in the proper 3:1 stoichiometric ratio at 500K. If the initial pressure is 1 atm, what is the % yield of ammonia? (% of maximum possible yield if all reactant were converted to product.)

Please use equilibrium constants to solve and show how to get concentration and percent yield. Please show step by step!

Use equation Kp = Kc(RT)^delta(n)