Consider the decomposition of ammonium hydrogen sulfide: NH4HS(s)NH3(g)+H2S(g) Initially, 1.00mol of NH4HS was placed in a sealed 1.50-L container. When equilibrium was reached, the concentration of NH3 was found to be 0.0134M. Then, the container volume was doubled to 3.00L and equilibrium was disturbed while the temperature was kept the same at 255C. a) (2 pts) Fill the ICE table for the first equilibrium with units. Then determine Kc. Show vour work below the table. b) (1pt) Calculate Kp. c) (1 pt) After the volume is doubled, which way should the reaction shift (reactant side or product side) to re-establish the equilibrium? No need to explain your answer. d) (1 pt) Fill in the ICE table for the second equilibrium with units after the volume was doubled. e) (3 pts) Calculate how many moles of NH3 remains after the second equilibrium is established