What volume of carbon dioxide will be produced if 10.3 g of glucose is fermented at 25°C and 100 kPa? (A) 1.30 L (B) 1.42 L (C) 2.57 L (D) 2.83 L - HSC - SSCE Chemistry - Question 17 - 2015 - Paper 1

During fermentation, 1 mole of glucose produces 2 moles of carbon dioxide (CO₂). Therefore:

$n_{CO₂} = 2 \times n_{glucose} = 2 \times 0.0571 \, mol \approx 0.1142 \, mol$

Using the ideal gas law, we can find the volume of CO₂ produced. At standard conditions (0°C and 100 kPa), 1 mole of gas occupies approximately 22.4 L.

At the given conditions, we adjust using the ideal gas law:

$V = nRT/P$

Where:

• $R = 8.314 \, J/(mol \, K)$ (ideal gas constant)
• $T = 25°C = 298 K$
• $P = 100 \, kPa = 100,000 \, Pa$

Plugging in values:

$V = \frac{0.1142 \, mol \times 8.314 \, J/(mol \, K) \times 298 \, K}{100,000 \, Pa} \approx 2.83 \, L$