Question

Which reactions are spontaneous?

i. C2H5OH(l) + 3O2(g) 2CO2(g) + 3H2O(l), G = –36.7 kJ
ii. 2C6H6(l) + 15O2(g) 12CO2(g) + 6H2O(l), G = –6,405 kJ
iii. CaCO3(s) CaO(s) + CO2(g), G = 13.0 kJ
iv. Ni(s) + Cl2(g) NiCl2(s), G = 1,130.28 kJ
A.) i and ii
B.) iii and iv
C.) i and iii
D.) ii and iv

Answer 1

If I am not mistaken, it woulf be i and ii are spontaneous since the values are negative.

Answer 2

Answer: The correct answer is option A.

Step-by-step explanation:

Gibbs's free energy is defined as the energy which is associated to the chemical reaction that can be used to do work. It is represented as "G".

When Gibbs's free energy is negative, the reaction is said to be spontaneous and when Gibbs's free energy is positive, the reaction is said to be non-spontaneous.

From the given options:

Reaction 1 and reaction 2 has negative Gibbs's free energy and hence, is considered as the spontaneous reactions.

Reaction 3 and reaction 4 has positive Gibbs's free energy and hence, is considered as the non-spontaneous reactions.

Therefore, the correct answer is Option A.