We’re given the following balanced reaction:
C12H22O11 + H2O + 3 O2 ⟶ 2 C6H8O7 + 4H2O
From the balanced equation, 1 mole of sucrose (C12H22O11) forms 2 moles of citric acid (C6H8O7).
Citric acid, C6H8O7, a component of jams, jellies, and fruity soft drinks, is prepared industrially via fermentation of sucrose by the mold Aspergillus niger. The equation representing this reaction is
C12H22O11 + H2O + 3O2 ⟶ 2C6H8O7 + 4H2O
What mass of citric acid is produced from exactly 1 metric ton (1.000 × 10 3 kg) of sucrose if the yield is 92.30%?
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Percent Yield concept. You can view video lessons to learn Percent Yield. Or if you need more Percent Yield practice, you can also practice Percent Yield practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Caughran's class at UGA.
What textbook is this problem found in?
Our data indicates that this problem or a close variation was asked in Chemistry - OpenStax 2015th Edition. You can also practice Chemistry - OpenStax 2015th Edition practice problems.