I'm really struggling with this Chemistry problem. Can someone please help me with this?

Question

When 45.0 mL of 4.8 M HCl reacts with an excess of Mg(OH)₂, how many grams of Magnesium Chloride (MgCl₂) are produced, given the unbalanced equation HCl + Mg(OH)₂ → H₂O + MgCl₂?

A. 0.11 moles

B. 0.11 g

C. 1.1 moles

D. 1.1 g

E. 10. g

Answer 1

2HCl + Mg(OH)₂ ==> 2H₂O + MgCl₂ ... balanced equation

moles HCl = 0.045 L x 4.8 mol/L = 0.216 moles

moles MgCl₂ formed = 0.216 moles HCl x 1 mol MgCl₂ / 2 mols HCl = 0.108 moles MgCl₂

mass MgCl₂ = 0.108 mols MgCl₂ x 95.2 g MgCl₂/ mol = 10. g MgCl₂ formed (answer E)

Answer 2

Well 45 ml of 4.8 M HCl gives 0.045 x 4.8 = 0.216 moles

From the equation this will give 0.216 moles of MgCl2

So find the molecular mass of MgCl2 and multiply by 0.216