As a sample of KNO3(s) is stirred into water at 25°C, the compound dissolves endothermically. Which — Thermodynamics Chemistry Question
Question
As a sample of KNO3(s) is stirred into water at 25°C, the compound dissolves endothermically. Which of the following best helps to explain why the process is thermodynamically favorable at 25°C?
A.
All endothermic processes are thermodynamically favorable.
B.
Stirring the solution during dissolution adds the energy needed to drive an endothermic process.
C.
The dissolution of KNO3(s) involves a decrease in entropy, which makes the process thermodynamically favorable.
D.✓ Correct
The entropy of the system increases during the dissolution, so TΔS is greater than ΔH.
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