Question

Which of the following is true for the Spontaneous process?

• A. $∆\mathrm{G}=0$
• B. $∆\mathrm{G}>0$
• C. $\mathrm{\Delta G}<0$
• D. $∆\mathrm{G}=\mathrm{T}∆\mathrm{S}$

Answer 1

The correct option is C

$\mathrm{\Delta G}<0$

The correct option is C.

Explanation for Correct option:

1. A spontaneous process is one that develops on its own under specific conditions without assistance from outside sources and moves in a specific direction.
2. Natural processes are always unplanned.
3. Gibb's free energy,

• $∆\mathrm{G}<0$ for a spontaneous process
• $∆\mathrm{G}>0$ for non-spontaneous process
• $∆\mathrm{G}=0$ for equilibrium process

Explanation for Incorrect option:

Option A:

It is an equilibrium reaction as $∆\mathrm{G}=0$ for the equilibrium process.

Option B:

it is not as spontaneous as $∆\mathrm{G}>0$ for the non-spontaneous processes.

Option D:

A negative value for $∆\mathrm{H}$ and a positive value for $∆\mathrm{S}$ both contribute toward achieving a negative value for $∆\mathrm{G}$ and a spontaneous reaction.

Final answer: $∆\mathrm{G}<0$ is true for the Spontaneous process.