Question

. The compound, C6H16N2 , is one of the starting materials in the production of nylon. It can be prepared from the following reaction involving adipic acid, C6H10O4 : C6H10O4(l) 2NH3(g) 4H2(g) £ C6H16N2(l) 4H2O(l) What is the percentage yield if 750. g of adipic acid results in the production of 578 g of C6H16N2 ?

Answer 1

97%

Step-by-step explanation:

The balanced equation for the reaction is given below:

C6H10O4(l) + 2NH3(g) + 4H2(g)

—> C6H16N2(l) + 4H2O(l)

Next, we'll calculate the mass of C6H10O4 that reacted and the mass of C6H16N2 produced from the balanced equation. This is illustrated below:

Molar Mass of C6H10O4 = (12x6) + (10x1) + (16x4) = 72 + 10 + 64 = 146g/mol

Molar Mass of C6H16N2 = (12x6) + (16x1) + (14x2) = 72 + 16 + 28 = 116g/mol

Next, let us calculate the theoretical yield of C6H16N2. This is illustrated below:

From the balanced equation above,

146g of C6H10O4 produced 116g of C6H16N2.

Therefore, 750g of C6H10O4 will produce = (750x116)/146 = 595.89g of C6H16N2.

Now, we can calculate the percentage yield of C6H16N2 as follow:

Actual yield = 578g

Theoretical yield = 595.89g

Percentage yield =?

%yield = Actual yield /Theoretical yield x100

%yield = 578/595.89 x 100

%yield = 97%

Therefore, the percentage yield of C6H16N2 is 97%

Answer 2

The percentage yield of adiponitrile (C6H8N2) produced is 104% (please pay attention to correct reaction equation below).

Step-by-step explanation:

During the production of nylon, the precursor produced from ammoniation of adipic acid (C6H10O4) is adiponitrile (C4H8N2). Hence the correct reaction equation is:

C6H10O4(l) + 2NH3 (g) → C6H8N2 (l) + 4H2O(l)

1 mole of C6H10O4 - 146.14 g (molar mass of adipic acid)

?? moles of C6H10O4 - 750 g

= 750 ÷ 146.14

= 5.13 moles of adipic acid are preset in the 750g used in the experiment.

But if mole ratio of reaction is 1:1, then 1 mole of adipic acid produces 1 mole of adiponitrile.

⇒ 1 mole of C6H8N2 - 108.14g

5.13 mole of C6H8N2 - ?? g

= 5.13 × 108.14 = 554.98g

∴ 554.98 g of adiponitrile should be produced during the reaction.

But percentage yield =
`(actual-yield)/(theoretical-yield)` × 100

=
`(578)/(554.98) * 100`

% Yield = 104%

NOTES:

• % yield can be greater than 100%, which means more sample was recovered from a reaction than predicted (which can occur in reactions as this where other product forming reactions occurred) or indicates presence of impurities.
• This steps can be used to solve alternatively for the formula provided in the question (C6H16N2), by solving with its molecular mass.