25g of NH3 is mixed with 4 moles of O2 in the given reaction: 4NH3(9) + 502(g) ---> 4N0(g) + 6H20(l)
a. What mass of NO is formed? b. Which is the limiting reactant?
c. What mass of H20 is formed?
To determine the mass of NO formed, we need to calculate the moles of NH3 and O2 present in the reaction and then use the stoichiometry of the reaction to find the moles of NO.
a. Moles of NH3:
Given: Mass of NH3 = 25g
Molar mass of NH3 = 17.03 g/mol (calculated by adding the molar masses of one nitrogen atom and three hydrogen atoms)
Moles of NH3 = Mass of NH3 / Molar mass of NH3
Moles of NH3 = 25g / 17.03 g/mol
Moles of NH3 ≈ 1.47 mol (rounded to two decimal places)
Moles of O2:
Given: Moles of O2 = 4 mol
According to the balanced equation, the ratio of NH3 to NO is 4:4, which means each mole of NH3 will produce one mole of NO.
Moles of NO = Moles of NH3
Moles of NO ≈ 1.47 mol
Mass of NO:
Molar mass of NO = 30.01 g/mol (calculated by adding the molar masses of one nitrogen atom and one oxygen atom)
Mass of NO = Moles of NO × Molar mass of NO
Mass of NO = 1.47 mol × 30.01 g/mol
Mass of NO ≈ 44.11 g (rounded to two decimal places)
Therefore, the mass of NO formed is approximately 44.11 g.
b. To determine the limiting reactant, we need to compare the moles of NH3 and O2 present.
Moles of O2: 4 mol
Moles of NH3: 1.47 mol
According to the balanced equation, the ratio of O2 to NO is 2:4, which means each mole of O2 will produce two moles of NO.
Moles of NO (from O2) = 2 × Moles of O2
Moles of NO (from O2) = 2 × 4 mol
Moles of NO (from O2) = 8 mol
Since the stoichiometry ratio shows that 4 moles of NH3 produce 4 moles of NO, but 4 moles of O2 can produce 8 moles of NO, the limiting reactant is NH3.
c. To find the mass of H2O formed, we need to use the stoichiometry of the reaction.
According to the balanced equation, the ratio of NH3 to H2O is 4:6, which means each mole of NH3 will produce 6 moles of H2O.
Moles of H2O (from NH3) = 6 × Moles of NH3
Moles of H2O (from NH3) = 6 × 1.47 mol
Moles of H2O (from NH3) ≈ 8.82 mol (rounded to two decimal places)
Mass of H2O:
Molar mass of H2O = 18.02 g/mol (calculated by adding the molar masses of two hydrogen atoms and one oxygen atom)
Mass of H2O = Moles of H2O (from NH3) × Molar mass of H2O
Mass of H2O ≈ 8.82 mol × 18.02 g/mol
Mass of H2O ≈ 158.9764 g (rounded to two decimal places)
Therefore, the mass of H2O formed is approximately 158.98 g.