Some CO₂ gas was kept in a sealed container at a pressure of 1 atm and at 273 K . This entire amount of CO₂ gas was later passed through an aqueous solution of Ca(OH)₂. The excess unreacted Ca(OH)₂ was later neutralized with 0.1 M of 40 mL HCl . If the volume of the sealed container of CO₂was x , then x is____cm³ (nearest integer).
[Given : The entire amount of CO₂ (g) reacted with exactly half the initial amount of Ca(OH)₂ present in the aqueous solution.]

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answer is 45.

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Detailed Solution

Let moles of CO₂=n moles of Ca(OH)₂ total initially =2n
excess Ca(OH)₂=n
gm equivalent of Ca(OH)₂= gm equivalent of HCl
$\begin{array}{l} n \times 2 = 0.1 \times \frac{40}{1000} \times 1 \\ n = 2 \times 10^{- 3} \\ Volume of {CO}_{2} = 2 \times 10^{- 3} \times 22400 = 44.8 {cm}^{3} \end{array}$