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(C) The chemical reaction for the decomposition of limestone is: $CaCO_{3(s)} \stackrel{\Delta}{\longrightarrow} CaO_{(s)} + CO_{2(g)}$ According to t

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$3.52$

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(C) The chemical reaction for the decomposition of limestone is: $CaCO_{3(s)} \stackrel{\Delta}{\longrightarrow} CaO_{(s)} + CO_{2(g)}$ According to the stoichiometry,$100 \ g$ of $CaCO_3$ produces $44 \ g$ of $CO_2$. Given mass of impure limestone = $10 \ kg$. Mass of pure $CaCO_3$ = $80 \%$ of $10 \ kg = 0.80 	imes 10 = 8 \ kg$. Since $100 \ kg$ of $CaCO_3$ yields $44 \ kg$ of $CO_2$,$8 \ kg$ of $CaCO_3$ will yield: $\frac{44}{100} 	imes 8 = 3.52 \ kg$ of $CO_2$.

The mass of $CO_2$ that will be obtained by heating $10 \ kg$ of $80 \%$ pure limestone $(CaCO_3)$ is ............... $kg$.

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