contestada

Chloe t. followed the procedure of this experiment to determine the empirical formula of a compound of iron (fe) and chlorine (cl). to do so, she added 2.15 g of zn to a solution containing 1.750 g of fe(x)cl(y). after the reaction was complete, she isolated 0.771 g of fe. the mass of cl in the fe(x)cl(y) solution is

Respuesta :

jacob193

[tex] m(\text{Cl}) = 0.979 \; \text{g} [/tex]

Explanation

The [tex] 1.750 \; \text{g} [/tex] sample contains only the atoms of

  • Iron, [tex] \text{Fe} [/tex], and
  • Chlorine, [tex] \text{Cl} [/tex]

Thus no matter what natural numbers [tex] x [/tex] and [tex] y  [/tex] are, [tex] m(\text{Fe}_x\text{Cl}_y) = m(\text{Fe}) + m(\text{Cl}) [/tex] shall holds.

Recall that zinc [tex] \text{Zn} [/tex] is more reactive than iron as seen in the reactivity series;  Adding zinc to the solution would reduce all iron atoms (regardless of the oxidation state, [tex] +2 [/tex] or [tex] +3 [/tex]) to their elementary form, hence displacing them out of the solution. [tex] 0.771 \; \text{g} [/tex] of iron was obtained and therefore [tex] m(\text{Fe}) = 0.771 \; \text{g} [/tex].

Thus

[tex] \begin{array}{lll}m(\text{Cl})& =& m(\text{Fe}_x\text{Cl}_y) - m(\text{Fe})\\ & = &1.750 \; \text{g}- 0.771\; \text{g}\\ &=&0.979\; \text{g}\end{array} [/tex]