Consider the reaction: 2HBr(g)—„H2(g) + Br26) Using standard thermodynamic data at 298K, calculate the free energy...

Question

Question

Consider the reaction: 2HBr(g)—„H2(g) + Br26) Using standard thermodynamic data at 298K, calculate the free energy change whe

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Answer 1

Answer #1

Given:

Gof(HBr(g)) = -53.45 KJ/mol

Gof(H2(g)) = 0.0 KJ/mol

Gof(Br2(l)) = 0.0 KJ/mol

Balanced chemical equation is:

2 HBr(g) ---> H2(g) + Br2(l)

ΔGo rxn = 1*Gof(H2(g)) + 1*Gof(Br2(l)) - 2*Gof( HBr(g))

ΔGo rxn = 1*(0.0) + 1*(0.0) - 2*(-53.45)

ΔGo rxn = 106.9 KJ

This is when 2 mol of HBr reacts as per given chemical equation.

For 1.84 moles of HBr, ΔGo rxn = 106.9 * 1.84 / 2 = 98.35 KJ

Answer: 98.35 KJ

Answer 2

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