Answer:
3L
Explanation:
Step 1:
The balanced equation for the reaction.
Fe2O3(s) + 6HCl(aq) → 2FeCl3(aq) + 3H2O
Step 2 :
Determination of the masses of HCl and Fe2O3 that reacted from the balanced equation. This is illustrated below:
Molar mass of Fe2O3 = 159.70g/mol
Molar mass of HCl = 36.46 g/mol
Mass of HCl from the balanced equation = 6 x 36.46 = 218.76g
From the balanced equation above,
159.70g of Fe2O3 reacted with 218.76g of HCl
Step 3:
Determination of the mass of HCl needed to react with 439g of Fe2O3. This is illustrated below:
From the balanced equation above,
159.70g of Fe2O3 reacted with 218.76g of HCl.
Therefore, 439g of Fe2O3 will react with = (439 x 218.76) /159.70 = 601.35g of HCl.
Step 4:
Conversion of 601.35g of HCl to mole. This is illustrated below:
Molar mass of HCl = 36.46 g/mol
Mass of HCl = 601.35g
Number of mole = Mass/Molar Mass
Number of mole of HCl = 601.35/36.46
Number of mole of HCl = 16.49 moles
Step 5:
Determination of the volume of the HCl that reacted.
This is illustrated below:
Mole of HCl = 16.49 moles
Molarity of HCl = 5.50 M
Volume =?
Molarity = mole /Volume
Volume = mole /Molarity
Volume = 16.49/5.5
Volume of HCl = 3L
Therefore the volume of HCl needed for the reaction is 3L
