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 positive and $\Delta$S is approximately zero"
C)"$\Delta$G is positive and $\Delta$S is negative"
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 positive and $\Delta$S is approximately zero" 
C)"$\Delta$G is positive and $\Delta$S is negative" 
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 an acid-base reaction is exothermic (releasing heat), then adding heat to the system (F1F1F1S1F1F1F10S) will shift the equilibrium towards the reactants (F1F1F1S1 and F1F1F1G1) to absorb the excess heat. Therefore, F1F1F1S1F1F1F10S will be approximately zero. As F1F1F1S1 is a weak acid and F1F1F1G1 is a strong base, the reaction F1F1F1S1 + F1F1F1G1 → F1F1F1S1F1F1F10S releases heat to the surroundings (exothermic), and therefore, F1F1F1S1F1F1F10G will be positive. Therefore, the correct choice is B.

For the Following Acid-Base Reaction,which Statement Is True Taking Δ\DeltaΔ S into Consideration? A)

For the Following Acid-Base Reaction,which Statement Is True Taking $\Delta$ S into Consideration?
A)