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/molB. N2 (g) + 3H2 (g) →2NH3 (g); ΔG∘f=-33.30 kJ/molC. 2C (s) + 2H2 (g) →C2H4 (g); ΔG∘f=68.20 kJ/molD. 2SO (g) + O2 (g) →2SO2 (g); ΔG∘f=-600.4 kJ/mol

Option B and D

Explanation:

The Gibb's free energy also referred to as the gibb's function represented with letter G. it is the amount of useful work obtained from a system at constant temperature and pressure. The standard gibb's free energy on the other hand is a state function represented as Delta-G, as it depends on the initial and final states of the system.

A feasible way to synthesize the product entails the spontaneity of the reaction.

The spontaneity of a reaction is explained by the standard gibb's free energy.

If Delta-G = - ve (the reaction is spontaneous)

if Delta - G = + ve (the reaction is non-spontaneous)

if Delta-G = 0 (the reaction is at equilibrium)

Hence the option (B and D) with negative Gibb's free energy are the reaction that are spontaneous.