100 mL of an 0.0100 M aqueous solution of calcium hydroxide will absorb carbon dioxide according to the equation $$\text{Ca(OH)}_2(aq) + 2\text{CO}_2(g) \rightarrow \text{Ca(HCO}_3\text{)}_2(aq)$$ The maximum volume, in mL, at STP of CO₂ that could be absorbed by the solution is A - VCE - SSCE Chemistry - Question 12 - 2002 - Paper 1

From the balanced equation, we see that 1 mole of Ca(OH)₂ reacts with 2 moles of CO₂. Therefore, the moles of CO₂ that can react with 0.00100 moles of Ca(OH)₂ is:

$\text{Moles of CO}_2 = 2 \times 0.00100 = 0.00200 \text{ moles}$

At STP, 1 mole of gas occupies 22.4 L. To find the total volume of CO₂:

$\text{Volume} = \text{Moles} \times 22.4 \text{ L/mole}$

Thus:

$\text{Volume of CO}_2 = 0.00200 \text{ moles} \times 22.4 \text{ L/mole} = 0.0448 \text{ L}$

Converting this to mL:

$0.0448 \text{ L} \times 1000 = 44.8 \text{ mL}$

The maximum volume of CO₂ that could be absorbed by the solution at STP is 44.8 mL.