Calculate the amount of carbon dioxide that could be produced when 1 mole of carbon is burnt in 16 g of dioxygen.

The correct option is 22g.

Let's calculate the amount of carbon dioxide produced step-by-step using stoichiometry.
First, we write the balanced chemical equation for the combustion of carbon in dioxygen (oxygen gas):
$$\text{C}\left(\text{s}\right)+{\text{O}}_2\left(\text{g}\right)\to {\text{CO}}_2\left(\text{g}\right)$$
From this balanced equation, we can see that:
1 mole of Carbon (C) reacts with 1 mole of dioxygen (O₂) to produce 1 mole of carbon dioxide (CO₂).

Next, let's determine the number of moles of the reactants available.
We are given:
1. Amount of carbon = 1 mole
2. Mass of dioxygen (O₂) = 16 g

The molar mass of dioxygen (O₂) is:
$$2\times 16\text{ g/mol}=32\text{ g/mol}$$
Now, we calculate the moles of dioxygen available:
$$\text{Moles of }{\text{O}}_2=\frac{\text{Mass of }{\text{O}}_2}{\text{Molar mass of }{\text{O}}_2}=\frac{16\text{ g}}{32\text{ g/mol}}=0.5\text{ moles}$$

Since 1 mole of carbon requires 1 mole of dioxygen for complete combustion, and we only have 0.5 moles of dioxygen, dioxygen (O₂) is the limiting reagent. It will be completely consumed in the reaction, and it limits the amount of product formed.

According to the stoichiometry of the reaction, 1 mole of O₂ produces 1 mole of CO₂.
Therefore, 0.5 moles of O₂ will produce 0.5 moles of CO₂.

Finally, we calculate the mass of 0.5 moles of CO₂ produced.
The molar mass of CO₂ is:
$$12+(2\times 16)=12+32=44\text{ g/mol}$$
The mass of CO₂ produced is:
$$\text{Mass of }{\text{CO}}_2=\text{Moles}\times \text{Molar mass}=0.5\text{ mol}\times 44\text{ g/mol}=22\text{ g}$$
Thus, the amount of carbon dioxide that could be produced is 22g.