The empirical formula of a compound is `CH_(2)O`. `0.0835` moles of the compound contains `1.0 g` of hydrogen Molecular formula of the compound is

The empirical formula of a compounds is CH_(2)O . 0.25 mole of this compound contains 1 gm hydrogen . The molecular formula of compound is :

The empirical formula of a gaseous compound CH_(2) . The density of the compound is 1.25 gm/lit at S.T.P. The molecular formula of the compound is 'X'

The empirical formula of a compound is CH_(2) . IF one mole of the compound has a mass of 42 g , its molecular formula is

The empirical formula of a compound is CH_2 . One mole of this compound has a mass of 42 grams. Its molecular formula is

The empirical formula of a compound is CH_(2)O .If the vapour density is 60, what would be the molecular formula of the compound?

The empirical formula of a compound is CH_2O_2 . What could be its molecular formula ?

0.1653 g aluminium reacts completely with 0.652 g chlorine to form chloride of aluminium. a. What is the empirical formula of the compound? b. If molecular mass of the compound is 267 amu, calculate the molecular formula of the compound.