Question

Consider the reaction: 12(g) + Cl2(g)—>21CI(g) Using standard thermodynamic data at 298K, calculate the free energy change whIodine AHºf (kJ/mol) AG°f (kJ/mol) Sº (J/mol K) 12(s) 0 0 116.1 12(9) 62.4 19.3 260.7 23.0 16.0 137 12(aq) I(g) 106.8 70.3 18Chlorine Cl(9) AHºf (kJ/mol) AG°f (kJ/mol) sº (J/mol K) 121.7 105.7 165.2 0 0 223.1 -23.0 121.0 Cl2(g) Cl2(aq) 7.0 ci (aq) -1

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Answer #1

Given:

Gof(I2(g)) = 19.3 KJ/mol

Gof(Cl2(g)) = 0.0 KJ/mol

Gof(ICl(g)) = -5.5 KJ/mol

Balanced chemical equation is:

I2(g) + Cl2(g) ---> 2 ICl(g)

ΔGo rxn = 2*Gof(ICl(g)) - 1*Gof( I2(g)) - 1*Gof(Cl2(g))

ΔGo rxn = 2*(-5.5) - 1*(19.3) - 1*(0.0)

ΔGo rxn = -30.3 KJ

This is when 1 mol of I2 reacts as per balanced equation.

For 1.950 moles of I2 reacting,

ΔGo rxn = -30.3*1.950 = 59.1 KJ

Answer: 59.1 KJ

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