If 10 g (90 % pure) limestone is heated,what | vedclass

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(B) The chemical reaction is: $CaCO_3(s) 	o CaO(s) + CO_2(g)$.Given mass of limestone = $10 \ g$.Since it is $90 \%$ pure,the mass of pure $CaCO_3 =

Vedclass · Accepted Answer

$2.016$

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(B) The chemical reaction is: $CaCO_3(s) 	o CaO(s) + CO_2(g)$.Given mass of limestone = $10 \ g$.Since it is $90 \%$ pure,the mass of pure $CaCO_3 = 10 	imes 0.90 = 9 \ g$.Molar mass of $CaCO_3 = 40 + 12 + (3 	imes 16) = 100 \ g/mol$.Moles of $CaCO_3 = \frac{9 \ g}{100 \ g/mol} = 0.09 \ mol$.According to the stoichiometry,$1 \ mol$ of $CaCO_3$ produces $1 \ mol$ of $CO_2$.Therefore,$0.09 \ mol$ of $CaCO_3$ produces $0.09 \ mol$ of $CO_2$.Volume of $CO_2$ at $NTP = 	ext{moles} 	imes 22.4 \ L/mol = 0.09 	imes 22.4 = 2.016 \ L$.

If $10 \ g$ ($90 \%$ pure) limestone is heated,what volume of $CO_2$ in liters will be obtained at $NTP$?

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