Answer:
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%
Answer:
The percentage yield of adiponitrile (C6H8N2) produced is 104% (please pay attention to correct reaction equation below).
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 = [tex]\frac{actual-yield}{theoretical-yield}[/tex] × 100
= [tex]\frac{578}{554.98} * 100[/tex]
% Yield = 104%
NOTES:
