A.)The equilibrium constant, Kp, for the following reaction is 0.110 at 298 K:


NH4HS(s) NH3(g) + H2S(g)


Calculate the equilibrium partial pressure of H2S when 0.371 moles of NH4HS(s) is introduced into a 1.00 L vessel at 298 K.


PH2S = ?? atm


B.) The equilibrium constant, Kp, for the following reaction is 0.497 at 500 K:


PCl5(g) PCl3(g) + Cl2(g)


Calculate the equilibrium partial pressures of all species when PCl5(g) is introduced into an evacuated flask at a pressure of 1.47 atm at 500 K .


PPCl5 = ?? atm

PPCl3 = ?? atm

PCl2 = ?? atm