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(D) The reaction of gas $A$ $(CO_2)$ with slaked lime $(Ca(OH)_2)$ forms a white precipitate of calcium carbonate $(CaCO_3)$:$Ca(OH)_2(aq) + CO_2(g) \

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$CO_2$ and $CO_2$

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(D) The reaction of gas $A$ $(CO_2)$ with slaked lime $(Ca(OH)_2)$ forms a white precipitate of calcium carbonate $(CaCO_3)$:$Ca(OH)_2(aq) + CO_2(g) \rightarrow CaCO_3(s) + H_2O(l)$On prolonged bubbling of $CO_2$,the precipitate dissolves due to the formation of soluble calcium bicarbonate $(Ca(HCO_3)_2)$:$CaCO_3(s) + H_2O(l) + CO_2(g) \rightarrow Ca(HCO_3)_2(aq)$On heating the resultant solution,the calcium bicarbonate decomposes to reform the white precipitate of $CaCO_3$ and releases gas $B$ $(CO_2)$:$Ca(HCO_3)_2(aq) \xrightarrow{\Delta} CaCO_3(s) + H_2O(l) + CO_2(g)$Thus,both gases $A$ and $B$ are $CO_2$.

Gas $A$ is bubbled through slaked lime when a white precipitate is formed. On prolonged bubbling,the precipitate is dissolved. On heating the resultant solution,the white precipitate reappears with the evolution of gas $B$. The gases $A$ and $B$ respectively are

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