All parts are 1 question. Thank you

Consider the following balanced equation: N2(g)+3H2(g)2NH3(g) 2.00mol of nitrogen are mixed with 4.00mol of hydrogen in a 0.400L container at an elevated temperature. At equilibrium 1.14mol of N2 remain. The equilibrium constant will be determined. First, The ICE table will be completed: What is x ? What is y, that is, how much hydrogen is used? (Hint, use one of the methods used in the balance equation review problems to do the calculation. Enter amount as a nesieive quantity An addtional hint is pvin en the fizezack) What is z, that is, how much ammonia is produce? What is the equilibrium constant, Keq ? (Remember to convert the number of moles to moles per liter or concentration in the equilibrium expression.) Answer: What is the number of nitrogen molecules in the balanced equation? (Refer to number 14)