Correct option is (d) 2.016
Amount of pure limestone (CaCO3) is 10 g of 90% sample = \(\frac{90}{100} \times 10 \) = 9g
Molecular mass of CaCO3 = 100
Thus 100 g of limestone gives 22.4 litres of CO2 at STP
9 g of limestone will give \(\frac{22.4}{100}\) x 9 = 2.016 lit