A 5.5 gm sample of an organic compound gave on quantitative analysis 1.4 gm of N and 3.6 gm of C and 0.5 gm of H. If Molecular mass of the compound is 55 then calculate E.F. and M.F.

3.0gms of an organic compound on combustion give 8.8 gm of CO_(2) and 5.4gm of water. The empirical formula of the compound is

0.156 gm of an organic compound on heating with fuming HNO_3 and AgNO_3 gives 0.235 gm of Agl . Calculate the percentage of iodine in the compound.

0.2g of an organic compound gave on combustion 0.55gm of CO_(2) and 0.0892g of H_(2)O .Calculate the percentage composition of Carbon in the compound.

A gas is found to contains 2.34 gm of nitrogen and 5.34 gm of oxygen simplest formula of the compound is :-

0.45 gm of an organic compound gave on combution 0.792 gm of CO_2 and 0.324gm of water. 0.24 gm of the same substance was Kjeldahlised and the ammonia liberated was absorbed in 50.0 ml of (M)/(8H_2SO_4) . The excess acid required 77.0 ml of (N)/(10)NaOH for complete neutralisation. Calculate the empirical formula of the compound.

An organic compound on analysis gave C=42.8% , H=720% , and N=50^ volume of 1 gm of the compoun was found to be 200 ml at STP. Molecular formula of the compound is:

40 gm of compound containing 4 nitrogen atoms per molecules on combustion gives 2.8 gm of N_2 gas.Molecular mass of compound is :

The empirical formula of anorganic compound is CH_2 .The mass of 1 mol of it is 42 gm.The molecular formula of the compound is: