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

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

nacl is added to the aqueous of what? ? in order to get a proper answer you have to specify the exact composition of the aqueous solution.

po-215 i got it right on the quiz