Acrylonitrile (C3H3N) Is The Starting Material For Many Synthetic Carpets And Fabrics. It Is Produced By The Following Reaction: 2C3H6 (g) + 2NH3 (g) + 3O2 (g) = 2C3H3N (g) + 6H2O (g) If 15.0 G C3H6, 10.0 G O2, And 5.00 G NH3 Are Reacted, What mass of the acrylonitrile can be produced assuming 100% yield?

11.072 g

Explanation:

2 C3H6 (g) + 2NH3 (g) + 3O2 (g) = 2C3H3N (g) + 6H2O (g)

molar mass of Acrylonitrile (C3H3N) = 53.06 g/mol

molar mass of C3H6 = 42.08 g/mol =

molar mass of NH3 = 17.031 g/mol

molar mass of O2 = 15.999 g/mol

mole of C3H6 = 15 g / 42.08 g/mol = 0.3565 mol

mole of NH3 = 5 g / 17.031 g/mol = 0.294 mol

mole of O2 = 10 g / (15.999 x 2g/mol) = 0.313

finding the limiting reagent be comparing the mole

2 mole of C3H6 react with 2 mole of NH3  and 3 mole of O2 to yield 2 mole of C3H3N

0.209 mole of  C3H6 react with 0.209 mole of NH3  and 0.313 oxygen

mass of Acrylonitrile (C3H3N) =  53.06 g/mol × 0.209 mol = 11.072 g

1 is the answer to this problem