Chemical ThermoDynamics (2nd half) - Aadi Patel

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Across
  1. 2. What does S stand for in ∆S?
  2. 3. Standard free energies of formation.
  3. 5. If ∆G > 0, the reaction in the forward reaction is ___________.
  4. 6. If ∆G < 0, the reaction is ___________ in the forward direction.
  5. 11. The branch of chemistry that deals with the relationship between heat and other forms of energy.
  6. 13. If ∆S is positive, for it to always be positive, ∆H has to be ___________.
  7. 14. This is equal to the internal energy of the system plus the product of pressure and volume.
  8. 15. The relationship between the free-energy changes under standard conditions for any process.
Down
  1. 1. G = H - TS
  2. 4. What does G stand for in ∆G?
  3. 7. If ∆G = 0, the reaction is at ___________.
  4. 8. The change in the free energy of the system for an isothermal process.
  5. 9. In any spontaneous process carried out at constant temperature and pressure, the free energy always ___________.
  6. 10. If ∆H and ∆S are both positive, it is only spontaneous at ___________ temperatures.
  7. 12. What does H stand for in ∆H?
  8. 16. When Q > K, the reaction proceeds spontaneously in the ___________ direction.