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 20 - 2015 - Paper 1

From the fermentation reaction:

$C_6H_{12}O_6 \rightarrow 2 CO_2 + 2 C_2H_5OH$

Each mole of glucose produces 2 moles of carbon dioxide. Thus, the moles of CO₂ produced:

$n_{CO_2} = 2 \times n_{glucose} = 2 \times 0.0572 \approx 0.1144 \text{ moles of CO₂}$

Using the Ideal Gas Law to find the volume of CO₂ at the given conditions:

$PV = nRT$

• P = 100 kPa,
• V is what we want to find,
• n = 0.1144 moles,
• R = 8.314 J/(mol·K) (converted to kPa·L/(mol·K)), and
• T = 25°C = 298 K.

Rearranging the Ideal Gas Law:

$V = \frac{nRT}{P}$

Calculating:

$V = \frac{0.1144 \times 8.314 \times 298}{100} \approx 2.83 L$

Based on our calculations, the volume of carbon dioxide produced is approximately 2.83 L. The correct answer is therefore:

(D) 2.83 L.