Practice question · Multiple choice
Gibbs free energy isolates the spontaneity criterion to system properties alone, yet it remains mathematically equivalent to the Second Law. Why does evaluating the system's enthalpy and entropy capture the total entropy change of the universe?
Hints
- Where does the heat released or absorbed by the system actually go?
- How does thermal transfer at constant temperature alter the entropy of a thermal reservoir?
Show the answer
C. The enthalpy term reflects entropy changes occurring in the surroundings
Why
Gibbs energy encapsulates the Second Law because quantifies the entropy transferred to surroundings at constant pressure. Assuming surroundings are negligible or redefining universal laws misinterprets how state functions link open boundaries.
Practise Gibbs Free Energy and Spontaneity
The app has 4 more questions on this lesson, and keeps your place in the course. Chemistry I is free to start.
More questions on Gibbs Free Energy and Spontaneity
- Diamond converts to graphite with Δ G < 0 at room temperature, yet diamonds do not visibly change. What does…
- A reaction has Δ H = +30 kJ/mol and Δ S = +100 J/mol/K. Set the temperature in kelvin above which it becomes…
- Sort each combination of signs by when the reaction is spontaneous.
- Which statements about Gibbs free energy are correct?
- A reaction with a positive enthalpy change can still be spontaneous.
- Complete the account of what Gibbs free energy does and does not tell you.
- Match each quantity to what it determines.