Based on the standard free energies of formation, which of the following reactions represent a feasible way to synthesize the product?

a. 2c(s)+h2(g)→c2h2(g); δg∘f=209.2 kj/mol
b. n2(g)+3h2(g)→2nh3(g); δg∘f=−33.30 kj/mol
c. 2c(s)+2h2(g)→c2h4(g); δg∘f=68.20 kj/mol
d. 2so(g)+o2(g)→2so2(g); δg∘f=−600.4 kj/mol

The correct answer are option B and D.

Explanation:

ΔG° = ΔH° - TΔS°

Where:

ΔG° = Gibbs's free energy of the reaction at temperature T.

ΔH° = Enthalpy of the reaction at temperature T.

ΔS° = Change in entropy of the reaction at temperature T.

From the given reaction, the reaction with value of  represents the a feasible way to synthesize the product. So, the correct answer are option B and D.

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