Question

Tutored Practice Problem 3.3.4 COUNTS TOWARDS GRADE Use reaction stoichiometry to calculate amounts of reactants and products. t GRAD use reaction stoichio The substances nitrogen monoxide and hydrogen gas react to form nitrogen gas and water Unbalanced equation: NO (+H2(g)N2 (g)H0 ) In one reaction, 49.5 g of H20 is produced. What amount (in mol) of H2 was consumed? What mass (in grams) of N2 is produced? mol H2 consumed g N2 produced Check & Submit Answer Show Approach

Answer 1

The balanced equation is

2 NO + 2 H₂ -----> N₂ + 2 H₂O

Number of moles of H2O = 49.5 g / 18.015 g/mol = 2.75 mol

From the balanced equation we can say that

2 mole of H2O is produced from 2 mole of H2 so

2.75 mole of H2O will be produced from

= 2.75 mole of H2O *(2 mole of H2 / 2 mole of H2O)

= 2.75 mole of H2

Therefore, the number of moles of H2 consumed would be 2.75

From the balanced equation we can say that

2 mole of H2O produces 1 mole of N2 so

2.75 mole of H2O will produce

= 2.75 mole of H2O *(1 mole of N2 / 2 mole of H2O)

= 1.38 mole of N2

mass of 1 mole of N2 = 28.0 g

so the mass of 1.38 mole of N2 = 38.6 g

Therefore, the mass of N2 produced would be 38.6 g