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?
All endothermic processes are thermodynamically favorable.
Stirring the solution during dissolution adds the energy needed to drive an endothermic process.
Dissolving the salt decreases the enthalpy of the system.
Dissolving the salt increases the entropy of the system.
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