0.246 g of an organic compound gave 0.198 g of `CO_2` and 0.101 g of `H_2O` on complete combustion calculate the percentage composition of Carbon and Hydrogen.

A 0.24 g of coumpound of oxgen and boron was found by analysis to contain 0.096 g of born and 0.144g of oxygen. Calculate the percentage composition of the compound by weight.

10g of CaCO3 on heating gave 4.4g of CO2 and X g of CaO. Applying law of conservation of mass , calculate the mass of CaO.

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 :

Complete combustion of 0.858 g of compound X given 2.64g of CO_2 and 1.26 g of H_(2)O. The lowest molecular mass X can have:

0.37 g of the compound gave 0.063 g of AgBr in Carius method. Determine the percentage bromine in the compound.

Calculate the volume of 4.4 g of CO_2 at S.T.P.

11.6g of an organic compound having formula C_n H_(2n+2) is burnt in excess of O_2(g) initially taken in a 22.41 litre steel vessel. Before reactio0n the gaseous mixture was at 273K with pressure reading 2 atm. Aftercomplete combustion and loss of considerable amount of heat, the mixture of product and excess of O_2 had a temperature of 546K and 4.6 atm pressure. The formula of organic compound is :