Calculate ∆H_rxn for the reaction of MgO(s) with HCl(g):

2 MgO(s)+ 4 HCl(g)⟶⟶ 2 MgCl₂(s) + 2 H₂O(l) ∆H_rxn = ?

using the following equations: (8 pts)

Mg(s) + 2HCl(g)⟶⟶ MgCl₂(s) + H₂(g) ∆H_rxn = -456.9 kJ

2Mg(s) + O₂(g) ⟶⟶2MgO(s) ∆H_rxn = -1203.2 kJ

2H₂O(l) ⟶⟶2H₂(g) + O₂(g) ∆H_rxn = 571.6 kJ

Use the ΔH°_f information provided to calculate ΔH°rxn for the reaction of MgO(s) with HCl(g): (6 points)

2MgO(s)+ 4HCl(g)⟶⟶ 2MgCl₂(s) + 2H₂O(l) ∆H_rxn = ?

ΔH°_f (kJ/mol)

MgO (g) -601.6

H₂O (l) -285.8

HCl(g) -92.3

MgCl₂ (l) -641.3

Suppose you carry out a precipitation by mixing 35 mL of 0.25 M barium chloride solution with 25 mL of 0.20 M aluminum sulfate solution. Calculate the mass in grams of the precipitate will form from the reaction.

Answer rating: 100% (QA)

Ans 3 Given 2 mgo s 4HCl 9 2 Mgch 8 2 H20les Attron u... View the full answer