A weighed sample of iron (Fe) is added to liquid bromine (Br₂) and allowed to react completely. The reaction produces a single product, which can be isolated and weighed. The experiment was repeated a number of times with different masses of iron but with the same mass of bromine (see graph below).

(a) What mass of Br₂ is used when the reaction consumes 2.0 g of Fe?
(b) What is the mole ratio of Br₂ to Fe in the reaction?
(c) What is the empirical formula of the product?
(d) Write the balanced chemical equation for the reaction of iron and bromine.
(e) What is the name of the reaction product?
(f) Which statement or statements best describe the experiments summarized by the graph?
(i) When 1.00 g of Fe is added to the Br₂, Fe is the limiting reagent.
(ii) When 3.50 g of Fe is added to the Br₂, there is an excess of Br₂.
(iii) When 2.50 g of Fe is added to the Br₂, both reactants are used up completely.
(iv) When 2.00 g of Fe is added to the Br₂, 10.8 g of product is formed. The percent yield must therefore be 20.0%.

Transcribed Image Text:

Mass of product (g) 12 10 8 6 4 2 0 0 1 2 Mass of Fe (g) 3 4