Question

Use reaction stoichiometry to calculate amounts of reactants and products. The substances ammonia and oxygen gas react to form nitrogen monoxide and water. Unbalanced equation: NH; (g) + O2(g) — NO(g) + H20 (g) In one reaction, 66.9 g of H2O is produced. What amount (in mol) of O2 was consumed? What mass (in grams) of NO is produced? mol O2 consumed g NO produced

Answer 1

4 NH3 + 502 - 4 NO + 640 66.99 6 moles of no consume 5 moles of Oz 6 x 18 g 1mal Ho consume 5x 32 g1 mal on 66.9 g 4,0 = 669 = 3.71 moles of tho 3.71 moles of n, o consume = 5 * 3.11 T 3.09 mole 0₂ 18 2.11 consume D 6 mole of ho is produced with 4 mole No 3.71 mole olho is produced with 4x3.71 6 = 2.47 moles of No 2.47 moles of No = 2.47 x 30 gimal mass of No = 74.2g