Laws of Chemical Combination
Two chlorides of iron were prepared.


I do not read that as: $\ce{FeCl_{n}}$ was prepared by two different methods, but as:


Reacting iron with dry chlorine gas yields $\ce{FeCl_{n}}$
Reacting iron with hydrogen chloride yields $\ce{FeCl_{m}}$


Apparently, iron is oxidized in both cases. 


What are the oxidants (what is reduced)?
Which of them is the stronger oxidant?
What is the stoichiometry (what are n and m)?


Could it be helpful to divide the amount of chloride produced by the amount of iron used? Would different numbers indicate which of the products has a higher chloride content? 


  (i) Calculate the mass of iron that reacted with 2.80 g of iron in each chloride.


Is it possible that they meant the same as indicated above, i.e.:

Calculate the amount of iron chloride that would have been produced from 2.80 g (instead of 4.50 g) iron in the first experiment and compare with the outcome of the second experiment.