. 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 ?

97%

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%

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