A sample of a halogenated hydrocarbon contains 0.48 g0.48\text{ g}0.48 g of carbon, 0.08 g0.08\text{ g}0.08 g of hydrogen, and 0.71 g0.71\text{ g}0.71 g of chlorine.
Show, by calculation, that the empirical formula of the compound is C2H4Cl\text{C}_2\text{H}_4\text{Cl}C2H4Cl.
The relative formula mass of the compound is 127127127. Deduce the molecular formula of the compound.
The displayed formula of another halogenated organic compound is:
H∣H−C−Cl∣H\begin{array}{ccccc} && \text{H} && \\ && | && \\ \text{H} &-& \text{C} &-& \text{Cl} \\ && | && \\ && \text{H} && \\ \end{array}H−H∣C∣H−ClDraw a dot-and-cross diagram of this compound. Show only the outer electrons.
80 exam-style questions on Edexcel IGCSE Chemistry Chemical formulae, equations and calculations. Each one has a worked solution and a mark scheme showing where the marks go.