Question

One of the intermediates in the synthesis of glycine from ammonia , carbondioxide and methane is aminoacetonitrile C2H4N2. The balanced chemical equation is 3CH4+5 CO2 + 8NH3 ---> 4C2H4N2 +10H2O. How much C2H4N2 could be expected from the reaction of 13.2 g CO2, 2.18 g NH3 and 17.0 g CH4

Answer 1

Answer:

mass of C₂H₄N₂ = 3.472 g

Explanation:

We have the following chemical reaction:

3 CH₄ + 5 CO₂ + 8 NH₃ → 4 C₂H₄N₂ + 10 H₂O

Using the masses given by the problem we calculate the number of moles for each reactant:

number of moles = mass / molecular weight

number of moles of CO₂ = 13.2 / 44 = 0.3 moles

number of moles of NH₃ = 2.18 / 17 = 0.13 moles

number of moles of CH₄ = 17 / 16 = 1.06 moles

We can see that the limiting reactant is ammonia NH₃. Now we can devise the following reasoning:

if         8 moles of NH₃ produces 4 moles of C₂H₄N₂

then    0.13 moles of NH₃ produces X moles of C₂H₄N₂

X = (0.13 × 4) / 8 = 0.062 moles of C₂H₄N₂

mass of C₂H₄N₂ = number of moles × molecular weight

mass of C₂H₄N₂ = 0.062 × 56 = 3.472 g