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, when an acid reacts with a base, the reaction will shift to form the weaker acid and weaker base. In this case, F1F1F1S1 is a strong acid and F1F1F1O10H is a weak acid. Therefore, the equilibrium will shift to the left to form more F1F1F1O10H, resulting in a decrease in the concentration of F1F1F1S1. This means that F1F1F1S1F1F1F10G is negative. However, since F1F1F1S1 is a strong acid and F1F1F1O10H is a weak base, the reaction will shift to form more F1F1F1O10H, resulting in an increase in the concentration of F1F1F1S1. This means that F1F1F1S1F1F1F10S is positive. Therefore, choice D is the correct answer.

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

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