For the following acid/base reaction which statement is true taking $\Delta$S into consideration?
A)"$\Delta$G is negative and $\Delta$S is approximately zero"
B)"$\Delta$G is negative and $\Delta$S is negative"
C)"$\Delta$G is positive and $\Delta$S is positive"
D)"$\Delta$G is negative and $\Delta$S is positive"
E)"None of these choices."

Question

For the following acid/base reaction which statement is true taking $\Delta$S into consideration? 
A)"$\Delta$G is negative and $\Delta$S is approximately zero" 
B)"$\Delta$G is negative and $\Delta$S is negative" 
C)"$\Delta$G is positive and $\Delta$S is positive" 
D)"$\Delta$G is negative and $\Delta$S is positive" 
E)"None of these choices."

Quizplus · Accepted Answer

According to Le Chatelier's Principle, if a stress is applied to a system in equilibrium, the system will adjust in the direction that minimizes the stress. In this acid-base reaction, F1F1F1S1 is the acid and F1F1F1S1O- is the base. If we add a strong acid to the reaction mixture, it will increase the concentration of H+ ions and shift the equilibrium to the left to reduce the stress. This means that the concentration of the acid (F1F1F1S1) will increase, while the concentration of the base (F1F1F1S1O-) will decrease. Therefore, F1F1F1S1F1F1F10G is negative as the equilibrium is shifted to the left, and F1F1F1S1F1F1F10S is positive as the concentration of the acid increases.

For the Following Acid/base Reaction Which Statement Is True Taking Δ\DeltaΔ

For the Following Acid/base Reaction Which Statement Is True Taking $\Delta$