At high temperatures and pressures, nitrogen will react with hydrogen to produce ammonia, as shown by the equation N2(g) + 3H2(g) --> 2NH3(g) For each of the following combinations of reactants, decide which is the limiting reactant. 1.25 moles of N2 and 3.65 moles of H2 44.0 g of N2 and 3.00 moles of H2 At high temperatures and pressures, nitrogen will react with hydrogen to produce ammonia, asshown by the equation_N2(g) +H2(g)>_NH3(g)For each of the following combinations of reactants, decide which is the limiting reactant.а.1.25 moles of N2 and 3.65 moles of H2|b. 44.0 g of N2 and 3.00 moles of H2

The balanced reaction taking place is given as, => N2 (g) + 3 H2 (g) ------> 2 NH3 (g) a) Given : Moles of N2 taken = 1.25 mol And moles of H2 taken = 3.65 mol From the above balanced reaction we can see that 1 mole of N2 requires 3 moles of H2 for complete reaction. Hence moles of H2 required = moles of N2 taken X 3 = 1.25 X 3 = 3.75 mol Since moles of H2 required is more than taken. Hence the limiting reactant is H2. b) Given : Moles of H2 taken = 3.00 And mass of N2 taken = 44.0 g Molar mass of N2 = Atomic mass of N X 2 = 14 X 2 = 28 g/mol Since mass = moles X molar mass => 44.0 = moles of N2 taken X 28 => moles of N2 taken = 1.57 mol approx. From the above balanced reaction we can see that 1 mole of N2 requires 3 moles of H2 for complete reaction. Hence moles of H2 required = moles of N2 taken X 3 = 1.57 X 3 = 4.71 mol Since moles of H2 required is more than taken. Hence the limiting reactant is H2.