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 ;

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

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 :

The following data were obtained from experiments to find the molecular formula of benzocaine, a local anaesthetic. (i) 3.54 g of it gave 8.49 g of CO_2 and 2.14 g of H_2O on complete combustion. (ii) 2.35 g of it was found to contain 0.199 g of nitrogen. (iii) The molecular mass of benzocaine was found to be 165 amu. Find the molecular formula of benzocaine.

An organic compound gave the following results on analysis, 0.2496 g of the compound gave 0.3168 g of CO_(2) and 0.0864 g of H_(2)O . Calculate the percentage of carbo and hydrogen in the compound.

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

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.

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.

0.2475g 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.