Question

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.	C(s)+O2(g)→CO2(g);	ΔG∘f=−394.4 kJ/mol
C.	2C(s)+2H2(g)→C2H4(g);	ΔG∘f=68.20 kJ/mol
D.	2CO(g)+O2(g)→2CO2(g);	ΔG∘f=−788.0 kJ/mol

Answer 1

Solution:

As we know... if G < 0 ...i.e. negative .... the reaction would be...both spontaneous and correspondingly feasible.....

And, if G > 0 ....i.e. positive ....the reaction wouldn't be ....neither spontaneous nor feasible...

Step - 1:

As we can see from the above Table ..... G < 0 ....i.e. negative for both reaction(s)... 'B' .....and 'D'.....making both of them feasible reactions, and we have the following....(given)

G^o_f = -394.4 kJ/mol ...... for reaction ....'B'....

And...

G^o_f = - 788.0 kJ/mol .... for reaction... 'D'...

Answer:

Therefore, based on the given and above shown data/informations, although both reaction 'B' and reaction 'D', represent a feasible way to synthesize the products .... the most feasible reaction should be.... reaction 'D'....... (i.e. the Answer)...

D.) 2CO (g) + O₂ (g) --------> 2 CO₂ (g)...... (reaction D)....G^o_f = - 788.0 kJ/mol...... (Answer)