Diluting concentrated sulfuric acid with water can be dangerous.The temperature of the solution can increase rapidly.What are the signs of $\Delta$_rH,$\Delta$_rS,and $\Delta$_rG for this process?

Question

Quizplus · Accepted Answer

When diluting sulfuric acid with water, the reaction is exothermic (releasing heat). Therefore, the enthalpy change (∆H) will be negative. The signs of entropy change (∆S) and Gibbs free energy change (∆G) will depend on the specific conditions of the reaction.
In this case, the temperature of the solution can increase rapidly, indicating that the entropy change (∆S) is positive (since the disorder increases with the increase in temperature). For the reaction to be spontaneous (∆G<0), both the enthalpy change (∆H) and entropy change (∆S) must be negative. Since we know that ∆H is negative and ∆S is positive, ∆G must be negative as well.
Therefore, the correct signs for the process are: 
∆H < 0 (since the reaction is exothermic)
∆S > 0 (since the temperature of the solution increases)
∆G < 0 (since the reaction is spontaneous) 
The only answer choice that has the correct signs for these changes is A.

Diluting Concentrated Sulfuric Acid with Water Can Be Dangerous Δ\DeltaΔ rH Δ\DeltaΔ

Diluting Concentrated Sulfuric Acid with Water Can Be Dangerous $\Delta$ _rH $\Delta$