`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 :

It has been found that 0.290 g of an organic compound containing C, H and O on complete combustion yielded 0.66 g of CO_2 and 0.27 g of H_2O . The vapour density of the compound is found to be 29.0. Determine the molecular formula of the compound.

0.45 g of a dibasic acid on combustion gave 0.44 g of CO_2 and 0.09 g H_2 O . The molecular mass of the acid is 90. Calculate the molecular formula. Suggest a structure for the acid.

An organic compound containing bromine gave the following results: (i) 0.125 g of the compound on complete combustion gave 0.1 g of CO_2 and 0.051 g of water. (ii) 0.185 g of the compound gave 0.32 g of AgBr. Sony Calculate the empirical formula of the compound.

Complete combustion of 0.858 g of compound X given 2.64g of CO_2 and 1.26g of H_2O The lowest molecular mass X can have ;

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.

0.29 g of an organic compound on combustion gave 0.66 g of CO_2 and 0.27 g of H_2 O . The percentage of carbon and hydrogen in the given compound respectively are

0.290 g of an organic compound containing C, H and O gave on combustion 0.270 g of water and 0.66 g of CO_(2) . What is empirical formula of the compound.

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

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

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.