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  4. What weight of CaCO3 must be decomposed to produce the sufficient quantity of carbon dioxide to convert 21.2 kg of Na2CO3 completely in to NaHCO3. [Atomic mass Na = 23, Ca = 40] CaCO3 → CaO + CO2 Na2CO3 + CO2 + H2O → 2NaHCO3

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Q. What weight of $CaCO_3$ must be decomposed to produce the sufficient quantity of carbon dioxide to convert $21.2\, kg$ of $Na_2CO_3$ completely in to $NaHCO_3$. [Atomic mass $Na = 23$, $Ca = 40$]
$CaCO_3 \to CaO + CO_2$
$Na_2CO_3 + CO_2 + H_2O \to 2NaHCO_3$

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Solution:

$
CaCO _{3} \rightarrow CaO + CO _{2}
$
$
100-56 \rightarrow 44
$
$Na _{2} CO _{3}+ CO _{2}+ H _{2} O \rightarrow 2 NaHCO _{3}$
$
106+18+44 \rightarrow 2 \times 84
$
Now you have $21.2 kg$ so $21200 \times \frac{44}{106}$. $=8.8 kg$ of $CO _{2}$ needed.
From eq. $188000 \times \frac{100}{44}$
$=20 kg$ of $CaCO _{3}$ is needed.