Problem: Acrylonitrile (C3H3N) is the starting material for many synthetic carpets and fabrics. It is produced by the following reaction:2 C3H6 (g) + 2 NH 3 (g) + 3 O2 (g) → 2 C3H3N (g) + 6 H2O (g)If 15.0 g C3H6, 10.0 g O 2, and 5.00 g NH 3 are reacted, what mass of acrylonitrile can be produced, assuming 100% yield?

FREE Expert Solution
  • Using the balanced equation provided, we can determine the mass of C3H3N based on the limiting reactant.
  • The limiting reactant is the reactant that will produce the least amount of C3H3N, we can determine this by using stoichiometry and the molar masses of each reactant:

MM of C3H6

C : 12.01 x 3 = 36.03

H: 1.01 x 6 = 6.06

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MM of C3H: 36.03 + 6.06  = 42.09 g/mol

MM of O2: 16 x 2 = 32 g/mol

MM of  NH3:

N: 14.01 x 1 = 14.01

H: 1.01 x 3 = 3.03 

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MM of NH3: 14.01 + 3.03 = 17.04 g/mol

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Problem Details

Acrylonitrile (C3H3N) is the starting material for many synthetic carpets and fabrics. It is produced by the following reaction:

2 C3H6 (g) + 2 NH 3 (g) + 3 O2 (g) → 2 C3H3N (g) + 6 H2O (g)

If 15.0 g C3H6, 10.0 g O 2, and 5.00 g NH 3 are reacted, what mass of acrylonitrile can be produced, assuming 100% yield?

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