At 25°C,ΔG°_fis -620 kJ/mol for SiCl₄(g)and -592 kJ/mol for MgCl₂(s).Calculate ΔG° for the reaction,SiCl₄(g)+ 2 Mg(s)→ 2 MgCl₂(s)+ Si(s)and determine if the reaction is spontaneous at 25°C if the pressure of SiCl₄(g)is 1 atm.

Question

Quizplus · Accepted Answer

We can use the equation ΔG°rxn = ΣνΔG°f(products) - ΣνΔG°f(reactants), where ν is the stoichiometric coefficient of each species in the balanced reaction and ΔG°f is the standard Gibbs free energy of formation.

For the given reaction, we have:

ΔG°rxn = 2ΔG°f(MgCl12) + ΔG°f(Si) - ΔG°f(SiCl14) - 2ΔG°f(Mg)

Substituting the given values, we get:

ΔG°rxn = 2(-592 kJ/mol) + 0 - (-620 kJ/mol) - 2(0) = -1184 kJ/mol + 620 kJ/mol = -564 kJ/mol

Since ΔG°rxn is negative, the reaction is spontaneous. Thus, the answer is C.

At 25°C,ΔG°f is -620 KJ/mol for SiCl4(g)and -592 KJ/mol for MgCl2(s).Calculate

At 25°C,ΔG°_fis -620 KJ/mol for SiCl₄(g)and -592 KJ/mol for MgCl₂(s).Calculate