100 mL of an 0.0100 M aqueous solution of calcium hydroxide will absorb carbon dioxide according to the equation Ca(OH)2(aq) + 2 CO2(g) ⇌ Ca(HCO3)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

According to the balanced equation, 1 mole of Ca(OH)₂ reacts with 2 moles of CO₂. Thus, the moles of CO₂ required are:

$n_{CO2} = 2 \times n_{Ca(OH)2} = 2 \times 0.00100 = 0.00200 \text{ moles}$

At standard temperature and pressure (STP), 1 mole of a gas occupies 22.4 L. Therefore, we can find the volume of CO₂ that can be absorbed:

$V = n_{CO2} \times 22.4 \text{ L/mol} = 0.00200 \times 22.4 = 0.0448 \text{ L}$

Converting this to mL: $0.0448 \text{ L} \times 1000 \text{ mL/L} = 44.8 \text{ mL}$

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