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6. The more disorder there is in the system, the

  • S is always a positive number
  • Higher the entropy
  • Decreases

7. In calculations concerning ΔG= ΔH - TΔS entropy is worked out using K

  • To convert C to K add 273 and the opposite to convert K to C
  • The entropy change that accompanies a reaction in the molar quantities as expressed in a chemical equation under standard conditions, all in standard states

8. The standard entropy S, of a substance is

  • The entropy content of one mole of the substance under standard conditions
  • S is always a positive number

9. The free energy change ΔG is

  • The balance between enthalpy, entropy, and temperature for a process: ΔG = ΔH - TΔS
  • The entropy change that accompanies a reaction in the molar quantities as expressed in a chemical equation under standard conditions, all in standard states

10. In calculations concerning ΔG= ΔH - TΔS 1, units must be the same for kJ/J

  • The units need to be the same, to convert ΔS to kJ K^-1 mol^-1 /1000
  • TΔS

11. Entropy increases during the changes in state that give more randomness, for example

  • solid (low entropy --> gas (high entropy)
  • Decreases
  • S is always a positive number

12. All substances posess some degree of disorder because particles are in constant motion, thus

  • S is always a positive number
  • Decreases

13. If a change makes a system more random ΔH is positive, and if a change makes a system more ordered, ΔS is

  • Negative
  • ΔSºreaction = ΣSº(products) - ΣSº(reactants)