How many milliliters of a 6.00 molar hydrochloric acid (hcl) solution would be needed to react completely with 100.0 grams of iron metal? 2fe (s) + 6hcl (aq) yields 2fecl3 (aq) + 3h2 (g) ?

The balanced equation for the above reaction is as follows;

2Fe + 6HCl - - > 2FeCl₃ + 3H₂

stoichiometry of Fe to HCl is 2:6

number of Fe moles reacted - 100.0 g / 56 g/mol = 1.79 mol

if 2 mol of Fe reacts with 6 mol of HCl

then 1.79 mol of Fe reacts with - 6/2 x 1.79 = 5.37 mol

the number of HCl moles required are 5.37 mol

if 6.00 mol of HCl are in 1 L volume of HCl solution

then volume required for 5.37 mol are in - 5.37 mol / 6.00 mol/L = 0.895 L

therefore volume required is 895 mL