Lime water turns milky when carbon dioxide gas is blown through it,with the formation of calcium carbonate. The reaction goes as follows:
CaO + CO2 turns CaCO3
If lime water is present in excess and calcium carbonate formed is 68g. Then, find the amount of carbon dioxide gas blown through the lime water in grams.

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Solution

$M o l e c u l a r m a s s o f C O_{2} = 12 + 2 (16) = 44 g M o l e c u l a r m a s s o f C a C O_{3} = 40 + 12 + 3 (16) = 100 g T h e g i v e n s t o i c h i o m e t r i c e q u a t i o n i s C a O + C O_{2} = C a C O_{3} 1 m o l e o f c a r b o n d i o x i d e g i v e s 1 m o l e o f C a C O_{3} i . e ., 100 g o f C a C O_{3} i s p r o d u c e d f r o m 44 g o f C O_{2} S o 68 g o f C a C O_{3} i s p r o d u c e d f r o m = \frac{44}{100} \times 68 = 29.92 g C O_{2}$

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Molecular mass of CO2 = 12 +2(16) = 44 gMolecular mass of CaCO3 = 40 +12 + 3(16) = 100 gThe given stoichiometric equation isCaO + CO2 = CaCO31 mole of carbondioxide gives 1 mole of CaCO3i.e.,100 g of CaCO3 is produced from 44 g of CO2 So 68 g of CaCO3 is produced from = 44100 × 68 = 29.92 g CO2