The mass of $CO_2$ produced by heating 20 g of 20% pure limestone, as per the equation given below, is:
$$ CaC

Question

The mass of $CO_2$ produced by heating 20 g of 20% pure limestone, as per the equation given below, is:
$$ CaCO_3(s) \xrightarrow{	ext{heat}} CaO(s) + CO_2(g) $$

Accepted Answer

1. **Calculate Mass of Pure Reactant:**
   - Total mass of limestone sample = $20 	ext{ g}$.
   - Percentage purity = $20\%$.
   - Mass of pure $CaCO_3 = 20 	ext{ g} 	imes \frac{20}{100} = 4 	ext{ g}$.
2. **Determine Molar Masses:**
   - Molar Mass of $CaCO_3 (1 	imes 40 + 1 	imes 12 + 3 	imes 16) = 100 	ext{ g mol}^{-1}$ [Class 12 Chemistry, Ch 1, Example 1.2].
   - Molar Mass of $CO_2 (1 	imes 12 + 2 	imes 16) = 44 	ext{ g mol}^{-1}$.
3. **Apply Stoichiometry:**
   - According to the balanced equation, $1 	ext{ mol } CaCO_3$ yields $1 	ext{ mol } CO_2$.
   - $100 	ext{ g } CaCO_3$ yields $44 	ext{ g } CO_2$.
   - Therefore, $4 	ext{ g } CaCO_3$ yields: 
     $$ 	ext{Mass of } CO_2 = \frac{44}{100} 	imes 4 = 1.76 	ext{ g} $$

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