The percent yield : = 79.87%
Further explanation
Percent yield is the comparison of the amount of product obtained from a reaction with the amount you calculated
General formula:
[tex]\tt \%yield=\dfrac{actual}{theoretical}\times 100\%[/tex]
An actual yield is the amount of product actually produced by the reaction. A theoretical yield is the amount of product that you calculate from the reaction equation according to the product and reactant coefficients or the maximum amount of product that can be produced from the reactant.
Given
991 g fructose
425 g ethanol
Required
The percent yield
Solution
Reaction
C₆H₁₂O₆(l)⇒ 2C₂H₆O(l) + 2CO₂(g)
mol fructose C₆H₁₂O₆ (MW=180,16 g/mol) :
= 991 g : 180.16 g/mol
= 5.5
From the equation, mol ratio of C₆H₁₂O₆ : C₂H₆O = 1 : 2, so mol C₂H₆O :
= 2/1 x mol C₆H₁₂O₆
= 2/1 x 5.5
= 11.55
Mass ethanol (MW=46,07 g/mol) :
= 11.55 x 46.07 g/mol
= 532.109 g
The percent yield :
= (425/532.109) x 100%
= 79.87%
Learn more
Percent yield from methane and oxygen reactions
https://brainly.ph/question/1472347
The percent yield of Al₂O₃
https://brainly.ph/question/1467820
Theoretical yield of the reaction
https://brainly.ph/question/2753293
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