When charcoal reacts in the presence of oxygen, carbon monoxide and carbon dioxide are produced according to the following chemical reactions - HSC - SSCE Chemistry - Question 20 - 2011 - Paper 1

In the first reaction, each mole of carbon produces 1 mole of carbon monoxide (CO).

Thus, using the moles of charcoal:

$\text{moles of CO} = 33.33 \text{ moles (from first reaction)}$

The molar mass of CO is approximately 28 g/mol.

Total mass of CO produced:

$\text{mass of CO} = 33.33 \text{ mol} \times 28 \text{ g/mol} = 933.24 ext{ g}$

In the second reaction, each mole of carbon produces 1 mole of carbon dioxide (CO₂).

Thus, using the moles of charcoal:

$\text{moles of CO₂} = 33.33 \text{ moles (from second reaction)}$

The molar mass of CO₂ is approximately 44 g/mol.

Total mass of CO₂ produced:

$\text{mass of CO₂} = 33.33 \text{ mol} \times 44 \text{ g/mol} = 1466.52 ext{ g}$

Now we can sum the masses of both gases produced:

Total gas mass = mass of CO + mass of CO₂

$\text{Total gas mass} = 933.24 ext{ g} + 1466.52 ext{ g} = 2399.76 ext{ g}$

Converting grams to kilograms:

Total gas mass = 2.4 kg

This closely matches the provided options and simplifies to 2.5 kg.

According to the calculations, the total mass of gas produced is approximately 2.5 kg.

Thus, the correct answer is (D) 2.5 kg.