Just a few questions I'm having trouble with. 1.Ammonia is formed from nitrogen and hydrogen according to the following equlibrium reaction: N2(g)+3H2(g)-->2NH3(g) The plant operates close to 700K, at which Kp is 1.00*10^-4 atm-2 and employs the stoiciometric ratio 1:3 of N22. At equilibrium, the partial pressure of NH3 is 50 atm. Calculate the partial pressures of the each reactant. 2.Ammonium carbamate (NH2COONH4) is a salt of carbamic acid that is found in the blood and urine of mammals. At 250c, Kc=1.58*10^-8 M^3 for the following equilibrium: NH2COONH4 (s) <---> 2NH3 (g) + CO2 (g) If 7.81g of NH2COONH4 is introduced into a 0.500L evacuated container, what is the total partial pressure inside the container at equilibrium at 250c? Thanks.