When glucose (C6H12O6) is completely fermented according to the reaction C6H12O6 → 2 C2H5OH + 2 CO2, what volume of hydrogen gas (H2) at STP could be produced from 256 g of glucose?

• A. 22.4 L
• B. 11.2 L
• C. 0 L
• D. 44.8 L

Answer: (C)

Verified step by step guidance

1. Identify the chemical reaction given: glucose (C6H12O6) is fermented to produce ethanol (C2H5OH) and carbon dioxide (CO2) according to the equation: \(\mathrm{C_6H_{12}O_6 \rightarrow 2\ C_2H_5OH + 2\ CO_2}\).
2. Note that hydrogen gas (H2) is not a product of this fermentation reaction. Therefore, no hydrogen gas is produced during this process.
3. Calculate the moles of glucose to confirm the amount of reactant: use the molar mass of glucose, which is approximately 180 g/mol, and calculate moles by \(n = \frac{\text{mass}}{\text{molar mass}}\).
4. Since the balanced equation does not include H2 as a product, the volume of hydrogen gas produced at STP is zero regardless of the amount of glucose fermented.
5. Conclude that the volume of hydrogen gas produced from 256 g of glucose under these conditions is 0 L.