If 120 mL of 2.8333 M aqueous HCl reacts stoichiometrically according to the balanced equation, how many milliliters of 4.43 M aqueous FeCl3 are produced?

Question

Fe2S3(s) + 6HCl(aq) → 3H2S(g) + 2FeCl3(aq)

Molar Mass (g/mol)
HCl 36.461
FeCl3 162.21
Density (g/mL)
-

Molar Volume (L)
22.4 at STP
Gas Constant
(L.atm.mol-1.K-1)
0.0821

I did

(2.8333mol x 120mL x 2mol FeCl3)/ (1000ml x 6mol)
got .113332mols and converted to mL by

(4.43mol x 1000) / .113332mol
and got 39089ml

i don't know if i did it correctly, the number seem pretty big

Answer 1

I did

(2.8333mol x 120mL x 2mol FeCl3)/ (1000ml x 6mol)
got .113332mols and converted to mL by
You are right to here with 0.1133 moles FeCl3. Then
M = moles/L and rearrange to
L = moles/M = 0.1133/4.43 = 0.02558 L = 25.58 mL. However, there is a flaw in the problem. Since you started with 120 mL of HCl, the final volume of the solution will be 120 mL and the molarity will be 0.1133 moles/0.120 L = 0.944 M OR if you evaporated the aqueous solution until 25.58 mL remained, then the solution would be 4.43 M.

(4.43mol x 1000) / .113332mol
and got 39089ml

i don't know if i did it correctly, the number seem pretty big