Question

As a chemical reaction proceeds over time spontaneously at a constant temperature, which statement is true:

A) ΔG0 approaches zero and ΔG remains unchanged

B) ΔG0 remains unchanged and ΔG approaches zero

C) ΔG0 approaches zero and ΔG approaches zero

D) ΔG0 remains unchanged and ΔG remains unchanged

E) ΔG0 decreases and ΔG remains unchanged

Please explain each answer choice in detail

Answer 1

∆G° is the standard Gibbs free energy change, and it is obtained under standard conditions . Hence it has a fixed value and does not changes.

Rather ∆G of the process or reaction changes, for an spontaneous process ∆G for a reaction is negative. And every process or reaction moves towards the attainment of equilibrium. And at equilibrium ∆G is Zero.

Hence the correct option will be Option 'B'.

Explaination of all the answer choices is based upon the above explanation.