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Using the equation for winemaking, how many liters of carbon dioxide would be produced with 287.62 g of glucose? Enter your answer as a number with the correct significant figures only.

a) 38.2 L
b) 45.6 L
c) 57.3 L
d) 69.8 L

Answer :

Final answer:

Calculating the volume of carbon dioxide produced from 287.62 g of glucose requires understanding the fermentation reaction's stoichiometry. Option D is the correct answer.

Explanation:

To answer the question regarding the volume of carbon dioxide produced from 287.62 g of glucose during fermentation, we need to understand the stoichiometry of the fermentation reaction. The balanced equation for the fermentation of glucose (C6H12O6) into ethanol (C2H5OH) and carbon dioxide (CO2) is:

C6H12O6 → 2 C2H5OH + 2 CO2

Given that 1 mole of glucose weighs 180.16 g and produces 2 moles of CO2, we first calculate the moles of glucose used:

Moles of glucose = 287.62 g / 180.16 g/mol = 1.596 mol

Thus, 1.596 mol of glucose produces 2 * 1.596 = 3.192 mol of CO2. Using the information that 1 mole of CO2 occupies 24.5 L at standard conditions, we find:

Volume of CO2 = 3.192 mol * 24.5 L/mol = 69.8 L.

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Rewritten by : Jeany

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