Chemistry
A hydride of nitrogen contains 87.5% percent by mass of nitrogen. Determine the empirical formula of this compound.
Related Questions
A compound with empirical formula AB has vapour density three times it's empirical formula weight. Find the molecular formula.
10.47 g of a compound contains 6.25 g of metal A and rest non-metal B. Calculate the empirical formula of the compound (At. wt of A = 207, B = 35.5)
A compound has O = 61.32%, S = 11.15%, H = 4.88% and Zn = 22.65%.The relative molecular mass of the compound is 287 a.m.u. Find the molecular formula of the compound, assuming that all the hydrogen is present as water of crystallisation.
The reaction between 15 g of marble and nitric acid is given by the following equation:
CaCO3 + 2HNO3 ⟶ Ca(NO3)2+ H2O + CO2
Calculate:
(a) the mass of anhydrous calcium nitrate formed
(b) the volume of carbon dioxide evolved at S.T.P.