1.5 g of ethane `(C_(2)H_(6))` on complete combustion gave 4.4 g of `CO_(2)` and 2.7 g of `H_(2)O`. Show that the results are in accordance to the law of conservation of mass.

3 g of ethane C_(2)H_(6) on complete combustion gave 8.8 g of CO_(2) and 5.4 g of water. Show that the results are in accordance with the law of conservation of mass.

In an experiment 5.0 g of CaCO_(3) on heating gave 2.8 g of CaO and 2.2 g of CO_(2) . Show that these results are in accordance to the law of conservation of mass.

0.22 g of a hydrogen (i.e., a compound conatining carbon and hydrogen only) on complete combustion with oxygen gave 0.9 g water and 0.44 g carbon dioxide. Show that these results are in accordance with the law of conservation of mass (atomic mass of C = 12, H = 1, O = 16) .

Complete combustion of 0.858 g of compound X gives 2.63 g of CO_(2) and 1.28 g of H_(2) O. The lowest molecular mass X can have

0.262 g of a substance gave, on combustion 0.361 g of CO_(2) and 0.147 g of H_(2)O . What is the empirical formula of the substance

44g of a sample on complete combustion given 88g CO_2 and 36g of H_2 O. The molecular formula of the compound may be :

44g of a sample on complete combustion given 88g CO_2 and 36g of H_2 O. The molecular formula of the compound may be :

0.2475g of an organic compound gave on combustion 0.4950 of CO_(2) and 0.2025g of H_(2)O calculate the % of C & H in it.

6g of a hydrocarbon on combustion in excess of oxygen produces 17.6g of CO_(2) and 10.8g of H_(2)O . The data illustrates the law of :

10.0 g of CaCO_(3) on heating gave 4.4 g of CO_(2) and x g of CaO. Applying law of conservation of mass calculate the mass of CaO.