How can I deduce the balance equation for magnesium sulphide using half equation method(ion-electron method)???

Question

Mateo Aguilar · Accepted Answer

Do you refer to #"steel-making..........."??#

Pig iron's sulfur is eliminated through the subsequent reaction with magnesium.

#Mg(l) + 1/8S_8(s) rarr MgS(s)#

According to what I've been told, the powdered magnesium sulfide floats on top of the liquid steel before being taken out of the blast furnace.

I would divide the various redox equations if I wanted to use half equations to illustrate this.

#"Oxidation (i):"# #Mg rarr Mg^(2+) rarr 2e^(-)#

#"Reduction (ii):"# #S +2e^(-) rarr S^(2-)#

#"Overall (i) + (ii):"# #Mg(s) + S(s) rarr MgS(s)#

Caleb Adams · Answer

undefined To deduce the balanced equation for magnesium sulfide (MgS) using the half-equation method (ion-electron method), follow these steps:

1. Write the half-equations for the oxidation and reduction reactions.
   Oxidation half-equation: Mg → Mg^2+ + 2e^-
   Reduction half-equation: S^2- + 2H^+ → H2S

2. Balance the number of atoms of each element in both half-equations.
   Oxidation half-equation: Mg → Mg^2+ + 2e^-
   Reduction half-equation: S^2- + 2H^+ + 2e^- → H2S

3. Balance the charges in both half-equations by adding electrons.
   Oxidation half-equation: Mg → Mg^2+ + 2e^-
   Reduction half-equation: S^2- + 2H^+ + 2e^- → H2S + 2e^-

4. Multiply the half-equations by suitable integers to make the number of electrons lost equal the number gained.
   Oxidation half-equation: Mg → Mg^2+ + 2e^-
   Reduction half-equation: S^2- + 2H^+ + 2e^- → H2S + 2e^-
   (Multiply the reduction half-equation by 1 to balance electrons)

5. Add the balanced half-equations together and cancel out any common terms to obtain the overall balanced equation.
   Mg + S^2- + 2H^+ → Mg^2+ + H2S