One of the intermediates in the synthesis of glycine from ammonia, carbon dioxide, and methane is aminoacetonitrile, C2H4N2.
How much C2H4N2 could be expected from the reaction of 14.9 g CO2, 2.11 g NH3, and 1.75 g CH4?

Explanation:

You must start by stating the chemical equation for the reaction of ammonia, carbon dioxide, and methane to produce aminoaceto nitrile.

1. Word equation:

Ammonia + Carbon dioxide + Methane → Aminoacetonitrile + Water

2. Balanced chemical equation:

3. Convert the mass of each reactant into number of moles:

Formula:

2.11g NH₃

14.9g CO₂

1.75g CH₄

4. Theoretical mol ratio

From the balanced chemical equation, using the coefficientes:

5. Limiting reagent

The available amounts of the reactants are:

Fom the theoretical mole ration, to react with 0.124 mol of NH₃ you would need:

Since there are 0.339 moles available, this is in excess.

Since there are 0.109 moles available, this is in excess too.

Hence, the limiting reagent is NH₃.

6. Yield

Use the theoretical ratio:

Convert to grams:

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